Electrochemical Conversion of Liquefied Forest Biomass Preliminary studies Tiago André Ribeiro da Silva Thesis to obtain the Master of Science Degree in Chemical Engineering Supervisors: Dr. José Augusto Dâmaso Condeço Dr. Diogo Miguel Franco dos Santos Examination Committee Chairperson: Prof. Maria Joana Castelo-Branco de Assis Teixeira Neiva Correia Supervisor: Dr. Diogo Miguel Franco dos Santos Members of the Committee: Dr. Rui Galhano dos Santos November 2018
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Electrochemical Conversion of Liquefied Forest Biomass
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Electrochemical Conversion of Liquefied Forest Biomass
Preliminary studies
Tiago André Ribeiro da Silva
Thesis to obtain the Master of Science Degree in
Chemical Engineering
Supervisors: Dr. José Augusto Dâmaso Condeço
Dr. Diogo Miguel Franco dos Santos
Examination Committee
Chairperson: Prof. Maria Joana Castelo-Branco de Assis Teixeira Neiva Correia
Supervisor: Dr. Diogo Miguel Franco dos Santos
Members of the Committee: Dr. Rui Galhano dos Santos
November 2018
I
Acknowledgments
I would like to thank my supervisors, Dr. José Condeço and Dr. Diogo Santos, for the opportunity
and guidance in the development of this work.
A word of appreciation to Professor Joana Neiva Correia for generously providing the laboratory
facilities and equipment necessary for the progress of this work.
I would also like to thank the members of the Materials Electrochemistry Group that, over the course
of this work, showed nothing but support and encouragement. A special word for Raisa Oliveira
and Aldona Balciunaite, thank you for all the time spent with me, all the assistance and, above all,
your friendship. To my colleague Inês Belo, thank you for the company during all those mornings
and afternoons we spent working in the laboratory, your presence made all the difference.
Also, a thank you to my colleagues, both past and present ones, and my friends that walked the
halls of this institute with me throughout these years.
Lastly, I would like to thank my family for everything, the support, love and all the sacrifices made.
Thank you for helping me reach this moment.
“Do not judge me by my successes, judge me by how many times I fell down
and got back up again”
- Nelson Mandela
II
Abstract
This work focuses on the use of different biomass, namely cork, pinewood and olive stones, to
produce bio-oil with the purpose of continuing further studies, which will provide preliminary information
regarding the suitability and potential towards the electrochemical conversion of bio-oils into industrially-
relevant compounds and the electrocatalytic upgrading of biomass-derived intermediates. Herein, the
liquefactions of the three biomass samples were performed and the obtained bio-oils were characterized
by several physicochemical methods (e.g., density, viscosity, conductivity and pH), followed by the
analysis of their electrochemical behavior. Both the anodic oxidation and the hydrogen evolution reaction
were evaluated at different potentials at room temperature using a Pt electrode. In the cyclic voltammetry
studies no redox peak was visible in the potential window between -2V and +2V. In the
chronoamperometry studies the current densities gradually decrease with time, stabilizing after 200
seconds. Two small-scale laboratory electrolyzers using nickel plate electrodes were assembled, one
being a single compartment cell and the other a cell with two-compartments separated by a membrane,
for the evaluation of the effect of an applied voltage of 2.5V on the composition of the bio-oils.
Electrolysis experiments were carried out up to 24 hours. The samples subjected to electrolysis were
analyzed by Attenuated Total Reflection-Fourier-transform Infrared Spectroscopy and Mass
Spectrometry, both before and after the electrolysis experiments, as to identify possible changes to the
samples chemical structure. The analyses show changes in the bio-oils composition, but the nature of
the actual changes occurring during the electrochemical process need further study.
Este trabalho foca-se no uso de diferentes biomassas, nomeadamente cortiça, pinho e caroço de
azeitona, para a produção de bio-óleo com o objetivo de efetuar estudos que irão providenciar
informação preliminar em relação à usabilidade e potencial para a conversão eletroquímica dos bio-
óleos em compostos com relevância a nível industrial e o melhoramento eletrocatalítico partindo dos
compostos intermediários. Foram efetuadas liquefações da biomassa e os bio-óleos obtidos foram
caracterizados por métodos físico-químicos (i.e., densidade, viscosidade, condutividade e pH), seguida
da análise do seu comportamento eletroquímico. Tanto a oxidação anódica como a reação da evolução
do hidrogénio foram avaliadas a vários potenciais à temperatura ambiente fazendo uso dum elétrodo
de platina. Na voltametria cíclica não foi visível nenhum pico redox na janela de potencial entre -2V e
+2V. A cronoamperometria mostrou que as densidades de corrente decrescem gradualmente com o
tempo, estabilizando ao fim de 200 segundos. Um par de eletrolisadores à escala laboratorial (elétrodos
de níquel) foram montados para avaliação do efeito da aplicação de uma tensão de 2.5V na composição
dos bio-óleos: uma célula de compartimento único, e uma célula de dois compartimentos divididos por
membrana. As amostras foram analisadas por Reflexão Total Atenuada-Espectroscopia no
Infravermelho por Transformada de Fourier e por Espectrometria de Massa, antes e após eletrólise, de
modo a identificar possíveis diferenças na sua estrutura química. As análises indicam diferenças nos
bio-óleos após serem submetidos a eletrólise. Serão necessários mais estudos para interpretar as
alterações que ocorrem durante o processo eletroquímico associado.
Palavras Chave: Liquefação de biomassa; Bio-Óleo; Eletrólise; Cortiça; Pinho; Caroço de Azeitona.
IV
Table of Contents
Acknowledgments .................................................................................................................................. I
Abstract .................................................................................................................................................. II
Resumo.................................................................................................................................................. III
Table of Contents .................................................................................................................................. II
List of Figures ....................................................................................................................................... VI
List of Tables ........................................................................................................................................ IX
List of Symbols and Abbreviations ..................................................................................................... X
Appendix ................................................................................................................................................ A
A. Mass Spectrometry ........................................................................................................ A
VI
List of Figures
Figure 1. Spatial arrangement of cellulose, hemicellulose and lignin in the cell walls of lignocellulosic
Figure 2. Structure of cellulose with a 1-4-β glycosidic bond, adapted from [1]. ................................ - 2 -
Figure 3. Sugar monomers typically found in Hemicellulose, adapted from [1]. ................................ - 2 -
Figure 4. The three monomers that form the lignin polymer along with their respective subunits, adapted
from [1]................................................................................................................................................. - 2 -
Figure 18. Scheme of the experimental procedure for the liquefaction’s product treatment. ........... - 20 -
Figure 19. Pt electrode, SCE and Pt coil used during the electrochemical characterization. .......... - 22 -
Figure 20. Diagram showing (A) the two emulsions, EAc with its distinct phases and EAlk, used in the
electrochemical experiments, with (B), showing the emulsions EAc’ and EAlk’, after 24 hours of
electrolysis in a single compartment cell, and (C), showing the emulsion EAc’’ and EAlk’’, after 24 hours
of electrolysis as a cathodic and anodic electrolyte, respectively, in a two-compartments cell. ....... - 23 -
Figure 21. Ni plates used as both anode and cathode in the electrolysis experiments. .................. - 25 -
Figure 22. Schematic of a two compartment cell with a membrane between each compartment, adapted
from [64]............................................................................................................................................. - 25 -
Figure 23. The effect of the addition of H2SO4 in the conductivity of sample of cork bio-oil. ........... - 30 -
Figure 24. Emulsions of cork bio-oil with (A) a 2 M H2SO4 aqueous solution, EAc, with visible separation
of the phases of the emulsion after 12 hours and an (B) a 2M KOH aqueous solution, EAlk, with no visible
Table XIV ATR-FTIR peak number, wavenumber range of values and corresponding assigned
functional groups, adapted from [70]. ................................................................................................ - 44 -
X
List of Symbols and Abbreviations
2-EH - 2-Ethylhexanol
[O] - Oxidized species
[R] - Reduced species
α - Charge transfer coefficient
A - Surface Area
ATR-FTIR - Attenuated total reflectance-Fourier-transform infrared spectroscopy
C - Molar concentration
CA - Chronoamperometry
CE - Counter-Electrode
C-OH - Cellulose fragment
CV - Cyclic voltammetry
D - Diffusivity
DEG - Diethylene glycol
DT - Dry torrefaction
E - Potential
EI - Electron ionization
ESI - Electron spray ionization
E0 - Standard potential of an electrode
EAc - Emulsion of cork bio-oil with a 2 M H2SO4 aqueous solution
EAc-Org - Upper layer of the Emulsion EAc, prominently organic
EAc-Int - Middle layer of the emulsion EAc
EAc-Aq - Bottom layer of the emulsion EAc, prominently aqueous
EAlk - Emulsion of cork bio-oil with a 2 M KOH aqueous solution
EAlk-Res - Viscous residue from the emulsion EAlk
EAc’ - Emulsion EAc after being subjected to electrolysis in a single compartment cell
EAc-Org’ - Upper layer of the Emulsion EAc’
EAc-Int’ - Middle layer of the emulsion EAc’
EAc-Aq’ - Bottom layer of the emulsion EAc’
EAlk’ - Emulsion EAlk after being subjected to electrolysis in a single compartment cell
EAlk-Res’ - Viscous residue from the emulsion EAlk'
EAc’’ - Emulsion EAc after being subjected to electrolysis as the catholyte in a two-compartments cell
EAc-Org’’ - Upper layer of the Emulsion EAc’’
EAc-Int’’ - Middle layer of the emulsion EAc’’
EAc-Aq’’ - Bottom layer of the emulsion EAc’’
EAlk’’ - Emulsion EAlk after being subjected to electrolysis as the anolyte in a two-compartments cell
EAlk-res’’ - Viscous residue from the emulsion EAlk’’
F - Faraday’s constant
HER - Hydrogen evolution reaction
HHV - Higher Heating Value
MS - Mass Spectrometry
i - Current
XI
j - Current density
jE - Current density at a specific potential, E
jp - Peak’s current density
jtf - Current density at the end of the electrolysis
j0 - Exchange current density
kB - Boltzmann’s constant
L-OH - Lignin fragment
LCO - Light cycle oil
LSV - Linear scan voltammetry
MS - Mass spectrometry
n1 - Electrolysis experiment in a single compartment cell of a sample of 1.5 M H2SO4 cork bio-oil
n2 - Electrolysis experiment in a single compartment cell of a sample of 1.5 M H2SO4 pinewood bio-oil
n3 - Electrolysis experiment in a single compartment cell of a sample of 1.5 M H2SO4 olive stones bio-oil
n4 - Electrolysis experiment in a single compartment cell of a sample of acidic emulsion, EAc
n5 - Electrolysis experiment in a single compartment cell of a sample of alkali emulsion, EAlk
n6 - Electrolysis experiment in a two-compartment cell with a sample of 2 M H2SO4 cork bio-oil as anodic electrolyte and a sample of 2 M H2SO4 aqueous solution as cathodic electrolyte.
n7 - Electrolysis experiment in a two-compartment cell with a samples of 2 M H2SO4 cork bio-oil as both anodic and cathodic electrolyte.
n8 - Electrolysis experiment in a two-compartment cell with a sample of acidic emulsion, EAc as anodic electrolyte and a sample of alkali emulsion, EAlk as cathodic electrolyte.
n - Number of electrons exchanged in an electrode reaction
na - Number of electron exchanged in the rate determining step
OCP - Open circuit potential
PEG - Polyethylene glycol
R - Universal gas constant
r - Radius of spherical particle
RE - Reference Electrode
rds - Rate-determining step
SCE - Standard calomel electrode
SHE - Standard hydrogen electrode
T - Temperature
t - Time
TsOH - p-Toluenesulfonic acid
η - Dynamic Viscosity
η - Overpotential
ν - Scan rate (mV s-1)
V - Volts
WE - Working Electrode
Wf - Final weight
Wi - Initial weight
WT - Wet torrefaction
Y - Yield
XII
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- 1 -
1. Introduction
1.1. Plant Biomass
The term biomass is used for all organic materials combustible in nature, mainly of plant and animal
origin. Plant biomass, also known as lignocellulosic biomass, encompasses residue of crop farming,
forestry industry and agro-industrial processing industries such as straw, bark, fruits and grains. This
Biomass is composed primarily of cellulose, hemicellulose and lignin, Figure 1. Dry biomass contains
roughly 40-45% cellulose, 25-35% hemicelluloses and 15-30% lignin [1–3].
Figure 1. Spatial arrangement of cellulose, hemicellulose and lignin in the cell walls of lignocellulosic
biomass [1].
Cellulose, Figure 2, is a linear polymer consisting of glucose monomers linked by 1-4-β glycosidic
bounds. The β bounds produces a linear conformation and enables the packing of numerous strands
into crystalline fibrils, as shown in Figure 1. Cellulose is the lignocellulosic polymer with highest degree
of polymerization at 10,000 or higher. The high molecular weight and low flexibility of cellulose chains
contributes to the cellulose polymer insolubility in water [1,2].
Hemicellulose is a polymer composed of C5 and C6 sugars, most typical xylose, arabinose, glucose,
mannose and galactose, Figure 3, with a degree of polymerization, around 100-200. Hemicellulose acts
as an amorphous matrix, holding the cellulose fibrils in place [1,2].
Lignin is a highly cross-linked, three-dimensional aromatic polymer consisting of three monomers,
coniferyl, sinapyl and p-coumaryl alcohols, Figure 4, mostly connected by C-C cross-links or ether
bounds. In the lignin polymer, the subunits are identified by their aromatic ring structure and are called
guaiacyl, syringyl and p-hydroxyphenyl subunits, respectively. Lignin composition differs between
- 2 -
softwood, hardwood and grasses, with softwood being composed mostly by guaiacyl while hardwood
contains a large quantity of syringyl groups [1,2].
Figure 2. Structure of cellulose with a 1-4-β glycosidic bond, adapted from [1].
Figure 3. Sugar monomers typically found in Hemicellulose, adapted from [1].
Figure 4. The three monomers that form the lignin polymer along with their respective subunits, adapted
from [1].
- 3 -
1.2. Thermochemical Conversion
Lignocellulosic biomass is an abundant resource that is commonly used as a source of energy by
direct combustion. However, several of its characteristics, such as low heating value, poor grindability
and high moisture content, are a disadvantage to its direct use as fuel [4]. Nowadays there are several
better alternatives for the efficient use of this renewable resource: sustainable production of liquid and
solid fuels, hydrogen, synthetic gases and valuable chemicals. The production of green chemicals and
clean, net zero carbon emission biofuels with an easy accessible, renewable resource has a promising
potential for development and is of extreme importance for or society and the environment. Some of the
most interesting processes to the exploitation of this resource and production of these valuable
compounds are the thermochemical conversions of biomass. These conversions consist on the
chemical transformation of organic matter at high temperatures. Thermochemical conversions, Figure
5, include processes like gasification, pyrolysis and liquefaction [5,6].
Figure 5. Classification of biomass’ thermochemical conversion technology.
Gasification is a process that can be used to produce a gas mixture from biomass such as wood or
agricultural wastes. The reaction is carried out at high temperatures in order to optimize the gas
production, resulting in small quantities of char and ash. The gasifying agent can be air, steam, air-
steam mixtures or oxygen mixtures. The gas, known as syngas, is usually a mixture of carbon monoxide,
hydrogen, methane, carbon dioxide and nitrogen, and its composition depends heavily on the
gasification process, the gasifying agent and the biomass composition [7,8]. Syngas from gasification is
part of the Indirect Liquefaction process, where liquid hydrocarbons are formed through Fischer-Tropsch
synthesis with Fe-, Co- or Ni-based catalysts [8].
Pyrolysis is the thermal decomposition of biomass in the absence of oxygen or air, under inert
atmosphere producing a liquid oil rich in oxygenated compounds, no condensable gases and solid char.
There are several pyrolysis processes, the two main processes being the slow pyrolysis and the fast
pyrolysis. In the slow pyrolysis the biomass is heated slowly and is primary used for the production of
char or charcoal that can be used as solid fuels [9]. In the fast pyrolysis the biomass is heated rapidly
so that it reaches the peak temperature before it decomposes. The primary objective of the fast pyrolysis
process is the production of bio-oil that can be used as a replacement for fuel oil or diesel in many
applications like boilers, furnaces and turbines. Due to the bio-oil proprieties, like high oxygen and water
- 4 -
content as well as high density and viscosity, making it unfavorable to use as transportation fuel several
methods were also developed to upgrade this bio-oil to conventional hydrocarbons fuels, like filtration,
solvent addition and catalytic methods, to cite a few [9–12].
Torrefaction is also a form of pyrolysis and it is known to be an effective process to pre-treat and upgrade
the biomass, improving its fuel properties. Nowadays there are two main different torrefaction processes,
dry torrefaction (DT) and wet torrefaction (WT). DT is conventionally a thermochemical pre-treatment of
biomass carried out either in an inert gas environment or in the presence of oxygen, carbon dioxide
atmosphere or a mixture of both, and in temperature range of 200-300 ºC, obtaining a solid product,
called biochar, as the main component. WT is a pre-treatment in hot water, at a pressure superior to the
saturated vapor pressure of the water, or hydrothermal media at temperatures of 180-260 ºC. In the WT
pre-treatment the main product is a solid called hydrochar. Both these pre-treatment techniques produce
solid fuels with better chemical, physical and fuel properties than raw biomass [4,9,13,14].
1.2.1. Direct Liquefaction
Direct liquefaction thermally decomposes solid biomass into predominantly liquid products, with
some char and gases, in the presence of a liquid solvent and an adequate catalyst. Usually, it is carried
out at moderate temperatures and pressures, ranging from 150 to 400 °C and 20 to 200 bar,
respectively. The operating pressure of a given direct liquefaction system is largely dictated by the vapor
pressure of the solvent, but it can be impacted by the vapor pressures of the products, as well.
The basic reaction pathways for the liquefaction process consists on the depolymerization of the
biomass into monomer units, which decompose by cleavage, dehydration, decarboxylation and
deamination, forming light fragments of small molecules, unstable and active. These light fragments
rearrange themselves by condensation, cyclization and polymerization into more stable molecules,
leading to new compounds [15,16]
Direct liquefaction is further divided into several subcategories delineated by the primary solvent used,
such as the hydrothermal liquefaction, in which water is the primary solvent, and the solvent liquefaction,
also known as solvolysis, in which other, usually organic, solvents are used instead.
Briefly, hydrothermal liquefaction, is a process where bio-oil is formed by thermochemical conversion in
water, that acts as a solvent, at high pressure and temperature. It is generally carried out at 250-400 ºC
and between 10 and 25 MPa. Biomass is mixed with water and a catalyst like sodium carbonate and
subjected to high pressure and temperatures. It has the advantage of skipping the drying step in the
biomass pre-treatment and of recovering any inorganics present in the biomass [2,5,17,18].
Solvolysis liquefaction is a process where biomass is dissolved in an organic solvent at moderate
temperatures, 120 ºC to 180 ºC, and atmospheric pressure. The organic solvents used are usually
polyhydric alcohols such as ethylene glycol, glycerol, ethanol, 2-ethylhexanol, polyethylene glycol and
so on. Acids, both strong and weak, can be used as catalyst in solvolysis liquefaction. Examples of acids
- 5 -
used are sulfuric acid, hydrochloric acid, p-toluenesulfonic acid and oxalic acid. The yield of the chemical
reactions in the liquefaction is affected by several variables, the most important being the concentration
and chemical composition of biomass, the solvent, the concentration and type of catalyst, temperature
and reaction time.
In relation to the composition of the biomass, the amount of cellulose and hemicellulose is not as
important in the conversion as the amount of lignin due to their simpler structures and easy
decomposition. Due to its complex structure, the higher the amount of lignin the lower the conversion,
and when thermally decomposed at temperatures above 252 ºC it forms free radicals of phenol through
repolymerization and condensation reactions originating solid residues [5,19]
For the type of solvent, simpler alcohols, like methanol, ethanol and propanol originate higher yields of
liquefaction, while alcohols with longer chains and organic acids leads to a higher amount of residue.
However, simpler alcohols have lower boiling point, which can lead to evaporation before the beginning
of the liquefaction. It is recommended that the solvent should be chosen such that it strongly reacts with
cellulose and, if possible, the solvent should be a product of the liquefaction itself, such as phenol and
its derivatives, simple alcohols or polyalcohols [20,21]. Besides the type of solvent, the ratio between
the amount of solvent and biomass is very important. High amounts of biomass may lead to a large
increase of viscosity which limits the reaction rate [20–23].
As the liquefaction is held in the presence of an organic or inorganic acid catalyst, sulfuric acid being
one of the most commonly used, the choice and concentration of catalyst is an important factor. Low
concentrations, such as 3%, promote the biomass degradation, however concentrations above the
optimal value may promote repolymerization and condensation reactions [20–22].
The temperature is also a very influential variable in the yield of the reaction, as the conversion of the
reaction increases with the temperature up to a certain optimal value. However, if the reaction is held at
temperatures higher than its optimal value, the amount of residues increases due to repolymerization
and condensation reactions as well as having an impact on other proprieties like viscosity and acidity
[19–22]
According to Zou et al. [23] there are three stages during biomass liquefaction with alcoholic solvents,
including biomass dehydration, volatilization of alcoholic solvents, and biomass alcoholysis. The
mechanisms of biomass liquefaction with alcoholic solvents, as proposed by Zou et al. in [23], can be
seen in Figure 6 and Figure 7.
Figure 6 presents the reaction pathway for cellulose with an acid catalyst and an alcohol as solvent. As
shown the degradation of cellulose and hemicellulose produces simple sugars like glucose and xylose
that by further reaction steps may produce aldehydes, ketones or esters. The depolymerization of lignin
(Figure 7) forms phenols that can react with the alcohol solvent to form different substances. Figure 8
shows the possible mechanisms of the reaction of fragments of biomass liquefaction with alcoholic
solvents, in (A) the cellulose fragments (C-OH) and (B) the lignin fragments (L-OH), with mono-, di- and
tri-alcohols. The image shows that the use of poly-alcohols promotes the formation of products of higher
molecular weight, the formation of heavy oils and higher quantity of residues [23].
- 6 -
A summary of some studies focused on liquefaction and their working conditions, specifically indication
of the biomass, solvent and catalyst used, the temperature and time of reaction, and the obtained
conversion or yield, can be seen in Table I. The higher reported conversion and higher yield were
achieved when using para-toluene sulfonic acid (pTsOH) as catalyst, maintaining the reaction
temperature in the order of the 160ºC.
Figure 6. Reaction pathway for the cellulose of an alcohol solvent and an acid catalyst [23].
Figure 7. Reaction pathway for lignin with alcohol solvent and acid catalyst [23].
- 7 -
Figure 8. Mechanism of reaction of liquefaction fragments with alcohol solvents. In (A), the mechanism
for cellulose fragments (HO-C) with mono-, duo- and tri-alcohol solvents, and in (B) the lignin fragments
(HO-L) with the alcohol solvents [23].
Table I. Summary of some works on the liquefaction process and its working conditions.
Author Ref. Biomass Solvent Catalyst Temp. /
ºC Time /
min Conversion /
%
Hassan et al. (2008)
[24]
Bagasse and
cotton stalks
PEG and glycerin
3% H2SO4 150 120 79% - 88%
Wang et al. (2009)
[25] Corn
stover Glycerol 3% H2SO4 160 60-480 75% - 88%
Hu et al. (2012)
[22] Soybean
straw Crude
glycerol 3% H2SO4 240 180 -
Zhang et al. (2013)
[26] Bagasse Glycerol /
PEG 3% H2SO4 150 120 90%
Yona et al. (2014)
[27] Cork
powder Glycerol /
PEG H2SO4 and
NaOH 150-200 60-180 95%
Soares et al. (2015)
[28] Cork
powder Glycerol /
PEG 3% - 4% H2SO4 150-160 60-80 70%
Braz et al. (2015)
[29,30] Pine
Sawdust DEG / 2-EH
0.5% - 3.5% p-TsOH, H2SO4,
AlCl3, Trichlorocyanu
ric acid
120-180 120 42% - 98%
Mateus et al. (2015)
[31–33] Cork dust DEG / 2-EH 3% p-TsOH 160 90 95%
Santos et al. (2015)
[34] Cork dust DEG / 2-EH 3% p-TsOH 160 5 96%
Lee et al. (2016)
[35] Empty
fruit bunch
Glycerol / PEG
3% H2SO4 150 120 63%
Haverly et al. (2018)
[16] Southern
yellow pine
LCO - 120 - 47% - 54%
- 8 -
Huang et al. [15] also did a summary of research progress in the effect of biomass and solvent type,
such as ethanol or mixed solvents, on the liquefaction process for biomass such as pine powder and
sawdust, rice and wheat straw, cornstalk and bagasse, to cite a few.
1.2.2. Bio-Oil
Bio-oils are liquid mixtures of oxygenated compounds containing carbonyl, esters, ketones and
phenolic functional groups, derived from depolymerization and fragmentation of cellulose, hemicellulose
and lignin.
These bio-oils are advantageous due to their elevated high heating value (HHV) in comparison with the
biomass used in their production [33], despite having lower values than conventional diesel.
Nonetheless, bio-oils can be used as a fuel in boilers, diesel engines or gas turbines for heat and
electricity generation [36].
As they are also rich in polyols and can be used to produce phenolic resins as well as several other
environmental friendly polymers and derivate products [25,37–39]. Santos et al. [40] developed a novel
formulation of a natural polymeric water-based adhesive designed to glue lignocellulosic surfaces, such
as wood and cork, from cork liquefaction. Esteves et al. [41] shows that it is possible to use bio-oil from
cork biomass liquefaction for the production of polyurethane foams.
Recently, the innovative generation of syngas uses the water electrolysis process with liquefied biomass
as a carbon source, necessary to obtain carbon monoxide and carbon dioxide [42]. Syngas has many
applications like the intermediate production of transport fuels, gas fuels and various chemicals.
Liquefied biomass can also be a source of other valuable chemicals, like the levulinic acid, furfural and
5-hydroxymethylfurfural, of extreme importance as an intermediate in the synthesis of many other
compounds [43]. Nilges et al. ([44]) made use of electrochemistry for the production of renewable
chemicals and biofuels, specifically a two-step electrochemical conversion of levulinic acid to octane via
valeric acid. The conversion of levulinic acid into hydrocarbons is usually achieved via multi-step
processes (under harsh conditions of temperature and pressure, 250 – 400 ºC and 10 – 35 bar of H2),
while the electrochemical reaction is performed at room temperature and in aqueous solutions, with a
natural phase separation allowing a simple separation of the hydrocarbon. In the electrochemical
processes, the selectivity for the reaction products are dependent on the electrolyte composition,
electrode material and current density [44,45].
The use of electrochemistry in the oxidation and reduction of organic species is not new. The
electrocatalytic oxidation of glucose, a product of the depolymerization of cellulose, into compounds
such as gluconolactone, a polyhydroxy acid used in cosmetics, is a well-studied process [46–50].
Electrochemical oxidation of D-mannose on platinum electrodes to produce mannonic acid, better
known as gluconic acid and used as a food addictive, is also a known process [51]. The electrochemical
oxidation of phenol has been studied for the synthesis of hydroquinone or benzoquinone and has been
reported as a means of waste water treatment [52,53]. Both the reduction of Xylose into Xylitol, a
sweetener accepted by medical science, and its oxidation into xylonic acid [54,55] are other examples
- 9 -
of the use of electrochemical processes in the conversion of chemicals present in the bio-oil into valuable
chemicals. Weinberg et al. ([56]) presents oxidation potentials, and some potential processes of
oxidation, of many organic compounds in several different electrolytes and electrodes
These studies come as no surprise since the advantages of the electrochemical process are numerous.
These advantages include an easier handling of the reaction media since in many cases only the
removal of solvent and electrolyte is required (for there is no chemical oxidant or its products to remove
from the reactor), the low cost of the process as, neglecting the initial cost of equipment, the power is
relatively inexpensive compared to chemical reagents and the yields are often adequate [56].
Despite the bio-oil promising potential for development and its importance as a green alternative to the
production of fuels, synthetic gases and many other valuable chemicals, to the best of our knowledge,
at the time of this work no significant studies were found on bio-oil electrochemical characterization nor
of the effects of its direct electrolysis. This work is a preliminary study focused on characterizing several
different bio-oils electrochemical behavior, with the intent of identifying the biomass under study, namely
cork pinewood and olive stones, with the highest potential to continue further studies regarding the
electrochemical conversion to industrial relevant compounds and the electrocatalytic upgrading of
biomass derived intermediates.
- 10 -
2. Electrochemistry
Electrochemistry is the branch of chemistry responsible for the study of the phenomenon of transfer
of electrons for the transformation of chemical energy into electric energy and vice versa. This
phenomenon happens in the interface between an electric conductor, the electrode, and an ionic
conductor, known as electrolyte. Electrodes are usually metals, both solid (as Pt, Ni, Au) or liquid (Hg,
amalgams), carbon (graphite) or semiconductor materials (Si). In the electrolyte, the current is
transported by the movement of the ions present in the solution, therefore, the more commonly used
electrolytes are aqueous solutions containing ionic species such as H+, Na+, Cl-, in water or in a non-
aqueous solvent [57,58]. These electrochemical reactions involve the charge transfer between the
electrolyte and the electrode, being heterogeneous processes, and can be either an oxidation or a
reduction reaction, depending on the species present in the electrolyte giving or taking electrons from
the electrode, respectively. Depending on the gain or loss of electrons by the reactional species, the
electrode is called the cathode or the anode [59].
2.1. Electrochemical Cell
Electrochemical cells are devices that consist of a vessel, commonly in glass (Pyrex and quartz),
Teflon or Nylon, and a set of electrodes. The electrodes present in the cell are connected to a power
source, such as a potentiostat/galvanostat, to apply the desired current or potential. The electrochemical
cells can be classified either as galvanic cells or electrolytic cells. Galvanic cells are cells that produce
electric energy from spontaneous redox reactions through applied potential difference in the cell.
Electrolytic cells are cells where the introduction of electric current enables the non-spontaneous
chemical reactions, inducing the conversion of electric energy in chemical energy [60]. Electrochemical
cells might present a varied number of arrangements. In this work will be used mainly arrangements
with two or three electrodes. Figure 9 displays both the referred arrangements, in (A) the common two
electrodes arrangement used in the electrolyzer, and in (B), the three electrodes arrangement frequently
utilized for fundamental studies. In the (A) arrangement with two working electrodes, the potential
difference is applied between both electrodes where, in a galvanic cell, the electrode with a more positive
charge is the cathode, and the other is the anode. These electrodes can be of the same material or of
different materials, being that their surface areas can be the same or vary, depending on the objective
and purpose. The (B) arrangement consists in the working electrode, the reference electrode and the
counter-electrode, also known as auxiliary electrode. In (B), the working electrode can work as either
anode or cathode, according to the applied potential difference between it and the reference electrode.
In this arrangement, the potential difference is recorded between the working electrode and the
reference electrode, and the electrons transfer happens between the working electrode and the counter-
electrode, avoiding possible disturbances to the reference electrode’s potential [58,61].
- 11 -
Figure 9. Schematic of a cell’s standard setup with (A) two electrodes and (B) three electrodes [62].
2.1.1. Electrodes
As previously mentioned, the electrodes used during this work can be divided in three groups, the
working electrodes, the reference electrodes and the counter-electrodes.
Working Electrodes
Working electrodes are the electrodes where the redox reaction of interest happens. Those can be made
of a varied number of materials, for instance noble metals, like Pt and Au, due to their natural resistance
to corrosion and oxidation, pure metals such as Ni or Hg, alloys like steel, graphite or semiconductor
materials like Si. Besides the material used, the electrode’s surface area is an important factor in
electrochemistry and both may vary depending on the purpose of the electrode [62].
Reference Electrodes
Reference electrodes are electrodes with a well-known, stable potential, used as a reference point in an
electrochemical cell for the control and measurement of the cell’s potential. The stability of the
electrode’s potential comes from the use of a redox system where the concentration of the components
or elements involved is constant. There are many different reference electrodes that can be used
depending on the characteristics of the cell, the working electrode and the electrolyte. The most
commonly used are: Standard Hydrogen Electrode (SHE), the Saturated Calomel Electrode (SCE) and
the Silver-Silver Chloride Reference Electrode [58,62,63].
Standard Hydrogen Electrode is used as standard reference point for standard electrochemical
reduction potentials, with its potential, Eº, assigned as zero volts at all temperatures by convention,
allowing the measure of the potential of any other electrode with respect to the SHE. The electrode is
composed of a Pt foil, connected to a Pt wire, immersed in a 1 M H+ aqueous solution, as exemplified
in Figure 10. The process starts when the electron charged Pt foil attracts a H+ from the solution to its
surface, forming a hydrogen atom, that combines with other hydrogen atom to create H2(g), that is
- 12 -
released from the system. For the system to work the surface of the Pt foil needs to be able to catalyze
Eq. [1] and a constant flow of H2 gas is required.
2 H3O+ + 2 e− → H2 + H2O Eq. [1]
Figure 10. Schematic of a SHE, adapted from [64].
Saturated Calomel Electrode is composed of solid Hg2Cl2 and liquid Hg immersed in a saturated KCl
solution, as shown in Figure 11. It is necessary to have the solution saturated as it allows for the
concentration of Cl- to be fixed by the KCl solubility, even if part of the solution is lost by evaporation,
ensuring the potential of the SCE remains constant. The potential is determined by the activity of Cl- in
equilibrium, according to:
1 2⁄ Hg2Cl2(s) + e− ⇌ Hg(l) + Cl
−(aq) Eq. [2]
Figure 11. Schematic of a standard SCE, adapted from [65].
- 13 -
Silver/Silver Chloride Electrode consists of solid silver wire coated in AgCl and submerged in a KCl
and AgCl solution, as shown in Figure 12. The electrode is based on Eq. [3], the redox couple between
AgCl and Ag, where the activity of the Cl- determines the potential. This a widely used reference
electrode because it is inexpensive and not as toxic as the SCE, which contains mercury.
AgCl(s) + e- ⇌ Ag+(aq) + Cl
-(aq) Eq. [3]
Figure 12. Schematic of a standard Ag/AgCl electrode, adapted from [65].
Counter-Electrodes
Counter-electrodes, also known as auxiliary electrodes, are used to close the electric circuit of the cell
by promoting the transfer of electrons between itself and the working electrode, through the external
circuit, avoiding any interference with the potential of the reference electrode provoked by said transfer.
As the electron transfer happens between it and the working electrode, its surface area is usually much
larger than the surface area of the working electrode to avoid it being a limiting factor. The substance
used in these electrodes is usually inert, such as Pt, Au or graphite, to avoid interfering in the process,
presenting itself in the shape of a mesh or coil to maximize its surface area, as shown in the figure
below:
- 14 -
Figure 13. Example of Pt counter-electrodes in the shape of a mesh and coil.
2.1.2. Potentiostat/Galvanostat
Potentiostat is a device used to control the potential difference between two electrodes, usually
between the working and the reference electrodes, according to a set-point value. The galvanostat is a
device used to control the flux of current in a cell. Usually, these devices already have coupled the
needed devices to measure both electric current and potential, also working as galvanometer and
potentiometer, respectively [59,62]. The following Figure 14 shows, as an example, the
potentiostat/galvanostat used in this work.
Figure 14. Potentiostat/Galvanostat Princeton Applied Research/EG&G Model 273A.
- 15 -
2.1.3. Open Circuit Potential (OCP)
The open circuit potential (OCP), is the potential of the working electrode measured in relation to
the reference electrode when the current is zero, this is, when no potential or current is being applied.
From this value it’s possible to find the ratio between the oxidized ([O]) and reduced ([R]) species of a
known redox reaction by applying the Nernst equation, Eq. [4], where R is the perfect gas constant, T
the absolute temperature, F the Faraday constant and n the number of electrons traded in the reaction
[57,58,63].
E = E0 −
RT
nFln (
[R]
[O]) Eq. [4]
2.2. Electrochemical Methods
In electrochemistry, there are numerous methods of analysis of a system. In this work, the
electrochemical methods addressed were the cyclic voltammetry (CV) and linear scan voltammetry
(LSV), where both methods study a system by applying a voltage scan, along with chronoamperometry
(CA) which studies the evolution of the current density with time at a fixed potential. The following topics
present a brief description of these methods.
2.2.1. Cyclic Voltammetry (CV)
Cyclic voltammetry (CV) is a technique that applies a linear voltage scan in both positive and
negative directions, at a specific scan rate, from an initial potential (E0) to a certain set point potential
(E1) and back again (E0 → E1 → E0). Thought the test, the current density for each potential is recorded,
tracing a current (i) vs. potential (E) curve and redox reactions appear as peaks in the curve at certain
potentials. CVs can be done at different scan rates, where each one will get a curve of similar shape,
with the difference being the total current, which increases with increasing scan rates. In slower scan
rates the diffusion layer has time to grow further from the electrode, and the flux to the electrode surface
is considerably smaller compared with faster rates. Figure 15 shows an example of a voltammogram
for the CV at different scan rates. In reversible reactions, Figure 15 (A), the peaks appear at a specific
potential, independently of the scan rate, as the electron transfer rate is superior to the mass transfer
rate. In irreversible reactions, Figure 15 (B), the opposite happens, showing an increase of the peak
potential with the scan rate.
- 16 -
Figure 15. CVs at several scan rates for (A), reversible reactions and (B) irreversible reactions.
2.2.2. Linear Scan Voltammetry (LSV) and Tafel Analysis
A similar method to CV, Linear Scan Voltammetry (LSV) scans the potential from an initial value to
a setpoint potential and records the resulting currents. In this work, the LSV is used for the analysis of
the cathodic zone where reduction reactions occur, such as the hydrogen evolution reaction (HER). The
analysis of the HER in bio-oils is important since it is one of the possible pathways for the valorization
of bio-oils while using the process of electrolysis.
Developed by Tafel, the Eq. [5], can be used for the analysis of the kinetics of reactions with a single
rate-determining step (rds). The equation relates the rate of an electrochemical reaction to the
overpotential, where a, the zero intercept, and b, the slope, are constants obtained from the linear
regression of the graphic representation of the overpotential, η, versus the logarithm of the current
density, log(-j), known as the Tafel Plot. The equation is usually used on high overpotential, in a range
between 100 mV and 300 mV, and in a region of the LSV where the current densities present a so-
called Tafel behavior, i.e., a linear relation between η and log(-j). The slope, b, and y-intercept, a,
obtained from Eq. [5] can be used to calculate the charge transfer coefficient, α, and the exchange
current density, j0, using Eq. [6] and Eq. [7], respectively, where R is the ideal gas constant, T is the
temperature in K, and F corresponds to the Faraday constant. The use of these parameters makes it
possible to compare the HER in different media.
η = E - E0 = a + b log(-j) Eq. [5]
b = 2.3 RT
αF Eq. [6]
a = b log(-j0) Eq. [7]
- 17 -
The charge transfer coefficient, α, defined as the fraction of the potential used in the electrochemical
reaction, this value can be used to determine the number of electrons exchanged in a reaction step
of a known system. For this it is necessary to resort to a linear regression, Eq. [8], where jp is the
current density of the peak, C is the concentration of the reduced species, D is the diffusion
coefficient and n is the number of electrons exchanged [57].
jp =
i
A = 2.99×10
5[(1-α)na]
1/2nC(Dν)
1/2 Eq. [8]
The exchange current density, j0, corresponds to the current where the forward and reverse
reactions are at state of equilibrium. It is a background current to which the net current observed at
various overpotentials is normalized, being an important variable in the rate of hydrogen evolution
reaction on metallic surfaces. Table II shows j0 values for different metals in a 1M H2SO4 solution,
where platinum shows to be the better metal for hydrogen evolution reaction, while the mercury is
the worst [57].
Table II. Comparison of j0 for hydrogen evolution reaction in 1 M H2SO4 [63].
Electrode material
-log (j0 / A cm-2)
Platinum 3.1
Iridium 3.7
Nickel 5.2
Gold 5.4
Titanium 8.2
Cadmium 10.8
Lead 12.0
Mercury 12.3
2.2.3. Chronoamperometry (CA)
Chronoamperometry (CA) is a potential-step method used to analyze the behavior of the current
density with time at a specific potential. In this method, the potential of the working electrode changes
instantly from an initial potential (E1) to a set potential (E2), as shown in Figure 16 (A). The
chronoamperogram corresponds to the current intensity registered with time, usually until it stabilizes,
Figure 16 (B). The zone of the graph where the current stabilizes is usually known as the diffusion-
controlled zone as in this zone the reaction is controlled by the diffusion of the species from within the
solution to the interface of the electrode.
- 18 -
Figure 16. (A), typical graph of a potential-step method and (B), example of a CA graph.
Chronoamperometry is a useful method to complement with other methods. It should only be used alone
when the process of the system in study is well known. Limited information about the identity of the
electrolyzed species can be obtained, from the ratio of the peak oxidation current versus the peak
reduction current, if present.
- 19 -
3. Experimental Methods
3.1. Bio-Oils and Reactants
All the bio-oil samples characterized in this study came from the liquefaction of ground plant
biomass, more specifically of cork, pinewood and olive stones biomass. In the solvolysis liquefaction,
the solvent used was 2-ethylhexanol (2-EH, 99%), from Acros Organic and the catalyst used was p-
toluenesulfonic acid (p-TsOH, 99%) from Acros Organic. Acetone (99.7%), from Sigma-Aldrich was
used in the treatment of the liquefaction solid residue. The reactants used in the electrochemical studies
was sulfuric acid (H2SO4, 95%), from Sigma-Aldrich, and potassium hydroxide (KOH, 90%), from Sigma-
Aldrich.
3.2. Solvolysis Liquefaction
The solvolysis liquefactions were performed with a procedure similar to ones found in the literature
[33]. The liquefactions were carried out in a glass reactor of 2 L equipped with mechanical stirring, a
thermocouple connected to the heating mantle, and a Dean-Stark separator/condenser. Figure 17,
below, displays the assembly used in the liquefaction. The solvolysis was performed with a weight ratio
of 1:2 biomass to solvent and 3 wt.% of catalyst, Eq. [9]. The reaction was run for four hours at 160 ºC,
after which the reactor was left to cool down at room temperature.
% catalyst = mcatalyst
msolvent
× 100 Eq. [9]
The procedure for the product treatment is exemplified in Figure 18. When cold, the reaction mixture
was subjected to centrifugation and sieving to separate the bio-oil from the solid residues. The solid
residues were thoroughly washed with acetone, subjected to centrifugation, filtration and then dried at
55 ºC in a hoven, and weighted. The bio-oil recovered from the solid residues was treated in a rotary
evaporator, at 40 ºC and low pressure, to remove the acetone from the bio-oil, and stored in separated
containers along with the remaining bio-oil for future use. The reaction conversion, defined in terms of
mass change, according to [21,29], is:
% C = (𝑊𝑖 – 𝑊𝑓)
𝑊𝑖
× 100 Eq. [10]
where Wi and Wf are the initial and final mass of the solid fraction, respectively.
- 20 -
Figure 17. Glass reactor in the heating mantle, at the bottom, coupled with a Dean-Stark
separator/condenser, on the left, a mechanical stirrer, up top, and the thermocouple controller on the
right.
Figure 18. Scheme of the experimental procedure for the liquefaction’s product treatment.
- 21 -
3.3. Bio-Oil Characterization
The bio-oils obtained by liquefaction were subject to several physicochemical methods to better
understand their characteristics and plan the following electrochemical studies with better rigor. The
characteristics analyzed were the density, viscosity, conductivity and pH, each briefly addressed in the
next topics. All samples subjected to electrochemical experiments were also subjected to attenuated
total reflection-Fourier-transform infrared spectroscopy (ATR-FTIR) and mass spectrometry (MS) with
the purpose of identifying possible changes in the bio-oils chemical composition related to said
experiments.
3.3.1. Density
Density or, to be more precise, the volumetric density of a substance is its mass for each unit of
volume. Density was verified as to obtaining a detailed characterization of the bio-oil. It was measured
with the aid of a pycnometer at room temperature.
3.3.2. Viscosity
Dynamic viscosity refers to the fluid’s internal resistance to flow when force is applied. It is a
characteristic taken in consideration as it directly affects the diffusivity of the particles in the bio-oil, as
shown by the well-known Stokes-Einstein equation, Eq. [11], where kB is the Boltzmann’s constant, T
is the absolute temperature, r is the radius of the spherical particle and η is the dynamic viscosity. This
has a direct impact on the electrochemical studies and electrolysis experiments when the reaction in the
interface of the electrode is controlled by the diffusion of particles in the electrolyte. The viscosity was
measured with a cone-and-plate viscometer from Research Equipment (London) Ldt., at 25 ºC.
D = kB × T
6 π × η × r Eq. [11]
3.3.3. Conductivity
Conductivity is a propriety that should be taken in consideration for electrolytes submitted to
electrochemical studies. As the redox reactions take place in the interface between the electrode and
the electrolyte, the contact between both phases should be adequately promoted for the efficient transfer
of the electrical currents. Conductivity was measured with a conductivimeter from HANNA Instruments,
model HI8733, at room temperature.
3.3.4. pH
The pH of the electrolyte is another propriety of extreme importance as certain electrodes can work
better or worse depending on the pH of the medium. Another factor is its effect on the redox reactions
in study, which may either be favored, or hindered by the pH of the medium. The pH value was measured
with a pH meter form HANNA Instruments, model HANNA pH20 at room temperature.
- 22 -
3.4. Electrochemical Experiments
The electrochemical experiments were performed at room temperature using a
potentiostat/galvanostat from Princeton Applied Research/EG&G, model 273A, shown in Figure 19,
controlled by PowerSuite software package. A platinum (Pt) electrode, from Metrohm, model 60305100
(A = 1 cm2) was used as the working electrode, a saturated calomel electrode (SCE) from HANNA,
model HI5412, was used as reference electrode and the auxiliary electrode was a Pt coil (A = 9.5 cm2),
as shown:
Figure 19. Pt electrode, SCE and Pt coil used during the electrochemical characterization.
A couple of small-scale laboratory electrolyzers were assembled with a couple of identical Ni electrodes
(A = 22 cm2), where it was used as both electrodes. The electrolyzers were a simple single compartment
cell and a two-compartment acrylic cell with an industrial membrane between compartments. The
samples studied where the cork, pinewood and olive stones bio-oil samples, both pure and with 3 M
H2SO4.
Another approach tried for the electrochemical experiments was adding an acid or alkaline aqueous
solution to the bio-oil, as the diagram in Figure 20 demonstrates. These mixtures formed emulsions of
bio-oil with aqueous solutions, in a 1:1 ratio. The diagram in Figure 20 (A) shows the two emulsions,
EAc being the emulsion formed by mixing the bio-oil with a 2 M H2SO4 aqueous solution, and EAlk, formed
by mixing the bio-oil with a 2 M KOH aqueous solution. The emulsion EAc was composed by three distinct
phases, the upper layer hereby known as EAc-Org, the middle layer EAc-Int and the lower layer EAc-Aq. The
emulsion EAlk did not form distinct layers, but formed a viscous residue, EAlk-Res. Part (B) of the diagram
in Figure 20 shows the emulsions EAc’, EAlk’ and their respective phases after 24 hours of electrolysis
in a single compartment cell with Ni plates as electrodes. And part (C), showing the emulsion EAc’’ and
EAlk’’ after 24 hours of electrolysis as cathodic and anodic electrolytes, respectively, in a cell with two
compartments divided by a porous membrane.
- 23 -
Figure 20. Diagram showing (A) the two emulsions, EAc with its distinct phases and EAlk, used in the
electrochemical experiments, with (B), showing the emulsions EAc’ and EAlk’, after 24 hours of
electrolysis in a single compartment cell, and (C), showing the emulsion EAc’’ and EAlk’’, after 24 hours
of electrolysis as a cathodic and anodic electrolyte, respectively, in a two-compartments cell.
All electrochemical experiments referred are addressed in the next topics.
3.4.1. Cyclic Voltammetry (CV)
Cyclic voltammetry was used to assess the liquefied biomass anodic oxidation as well as to
evaluate the HER potential in the bio-oil. The CV scans were performed using a Pt electrode in the
potential window between -2 V and +2 V at a scan rate of 50 mV s-1. The CVs were run using bio-oil
samples of cork, pinewood and olive stones bio-oil samples, both pure and with 3 M H2SO4 as well as
the acidic emulsion EAc and the alkali emulsion EAlk.
- 24 -
3.4.2. Linear Scan Voltammetry (LSV) and Tafel Analysis
Linear scan voltammetry was used specifically to assess the samples cathodic processes, more
specifically, the HER. The LSV scans were performed in the samples of cork, pinewood and olive stones
with 3 M H2SO4, from the OCP up to potential of -2 V, at a scan rate of 50 mV s-1. These LSVs were
used to get the Tafel plots for the study of the HER.
3.4.3. Chronoamperometry (CA)
Chronoamperometry measurements were made by applying a range of potentials from 0.7 V to
1.3 V in the anodic zone and from -0.5 V to -1.3 V in the cathodic zone, for 200 seconds. The samples
subject to analysis were the cork, pinewood and olive stones bio-oil samples, both pure and with 3 M
H2SO4.
3.4.4. Electrolysis Experiments
Small-scale laboratory electrolyzers were assembled using a pair of identical Ni plates (A = 22 cm2)
as electrodes, see Figure 21. The experiments were performed using cork, pinewood and olive stones
bio-oil samples and an applied potential of 2.5 V at room temperature. It was used both a simple single
compartment cell with a volume of 150 cm3 and a two-compartment acrylic cell, each compartment with
a volume of 80 cm3, with an industrial membrane separating both compartments, as seen in Figure 22.
The electrolysis experiments were performed up to 24 hours using a BK Precision (model 1621A), and
a summary of the different electrolysis experiments run on each cell can be seen on Table III, below.
In the single compartment cell, the samples subjected to electrolysis were a sample of cork bio-oil with
1.5 M H2SO4, n1, a sample of 1.5 M H2SO4 pinewood bio-oil, n2, a sample of 1.5 M H2SO4 olive stones,
n3, an emulsion EAc, of cork bio-oil with a 2 M H2SO4 aqueous solution, n4, and an emulsion EAlk, of
bio-oil with 2 M KOH aqueous solution, n5.
In the two-compartment cell, Figure 22, several different electrolytes were used in both the anodic and
cathodic compartment. In experiment n6, an aqueous solution of 2 M H2SO4 was used as electrolyte in
the cathodic compartment, and a sample of cork bio-oil with 2 M H2SO4 as electrolyte in the anodic
compartment. In electrolysis experiment n7, was using a sample of cork bio-oil with 2 M H2SO4 as
electrolyte in both compartments to try to isolate the possible redox reactions happening at each
electrode.
In experiment n8, the emulsion EAc was used as electrolyte in the cathodic compartment and the
emulsion EAlk was used in the anodic compartment. The electrolysis experiments of the emulsions were
performed with continuous mechanical agitation to ensure the emulsion remained as “homogeneous”
as possible.
- 25 -
Table III. Electrolysis experiments run on each cell, the electrolyte used and their working conditions.
Single Compartment Cell
Electrolysis Electrolyte Duration / h Agitation
n1 1.5 M H2SO4 cork bio-oil 14 No
n2 1.5 M H2SO4 pinewood bio-oil 14 No
n3 1.5 M H2SO4 olive stones bio-oil 14 No
n4 Emulsion EAc 24 Yes
n5 Emulsion EAlk 24 Yes
Two Compartments Cell
Electrolysis Anodic Electrolyte Cathodic electrolyte Duration / h Agitation
n6 2 M H2SO4 cork bio-oil 2 M H2SO4 aqueous solution 14 No
n7 2 M H2SO4 cork bio-oil 2 M H2SO4 cork bio-oil 14 No
n8 Emulsion EAlk Emulsion EAc 24 Yes
Figure 21. Ni plates used as both anode and cathode in the electrolysis experiments.
Figure 22. Schematic of a two-compartment cell with a membrane between each compartment, adapted
from [66].
- 26 -
3.5. Bio-Oil Analysis: Electrolysis Experiments
The next sub-chapters focus on the bio-oil analysis before and after the electrochemical studies.
The analysis used in this approach were the attenuated total reflection-Fourier-transform infrared
spectroscopy (ATR-FTIR) and the mass spectrometry (MS). The ATR-FTIR and MS analysis were used
in several cork bio-oil samples subjected to electrolysis, both before and after, with the purpose of
identifying possible changes in the functional groups present.
3.5.1. Attenuated total reflection-Fourier-transform Infrared Spectroscopy (ATR-FTIR)
Fourier-transform infrared spectroscopy (FTIR) is a technique used to obtain an infrared spectrum
of absorption or emission of a solid, liquid or gas. The infrared spectrum absorption peaks correspond
to the frequencies of vibrations between the bonds of the atoms making up the material. As each
different material is a unique combination of atoms, each compound produces a unique infrared
spectrum. Therefore, infrared spectroscopy can result in a positive identification, a qualitative analysis,
of every different kind of material. In addition, the size of the peaks in the spectrum is a direct indication
of the amount of material present. An attenuated total reflection accessory operates by measuring the
changes that occur in a totally internally reflected infrared beam when the beam comes into contact with
a sample [67–69].
Several cork bio-oil samples were subjected to ATR-FTIR analysis to identify the possible changes in
the samples after being subjected to electrolysis. The samples analyzed, before and after the
electrolysis experiments, were a cork bio-oil sample with 2 M H2SO4 as well as samples of the emulsions,
EAlk’, EAlk’’, EAc-Org’, EAc-Org’’, EAc-Aq’ and EAc-Aq’’.
ATR-FTIR spectroscopic analysis was performed using a Thermo Nicolet Nexus apparatus with an ATR
accessory. Each spectrum was obtained by the average of 32 scans with a resolution of 8 cm -1.
3.5.2. Mass Spectrometry (MS)
Succinctly, mass spectrometry (MS) is an analytical technique that ionizes chemical compounds
and sorts the ions formed based on their mass-to-charge ratio. The mass spectrum is a plot of the ions
signal as a function of the mass-to-charge ratio and is used to determine the masses of the present
species. The atoms or molecules in the sample can be correctly identified by correlating known masses
to the masses determined by MS. Depending on the nature of the ionization process, and the nature of
the atoms and molecules in the sample, different ion types can be formed. The most common way in
which ions are produced in a mass spectrometer is through the loss of an electron by the initial collision
of a gaseous atom or molecule with an electron in a process known as electron impact or electron
ionization (EI). However, the ionization method used in this MS is the electron spray ionization (ESI), in
- 27 -
which a high voltage is applied to a liquid to create an aerosol. Simultaneously, increasing the
temperature originates desolvation. This method is especially useful in producing ions from
macromolecules because it overcomes the propensity of these molecules to fragment when ionized. As
the polarity of the voltage applied to the detector is opposite to that of the ions in order to attract them
to the ion detector, the detection of both positive and negative ions simultaneously is not possible, each
mass spectrum being either positive or negative [70].
The first samples subjected to MS were the original cork bio-oil, the emulsion phases EAc-Org, EAc-Int and
EAc-Aq, as well as the emulsion EAlk and the residue EAlk-Res. The emulsion phases EAc-Org’, EAc-Int’, EAc-
Aq’, EAlk’ and EAlk-Res’, were also analyzed by MS and compared with the originals to identify possible
changes caused by said electrolysis experiment.
The instrument used in the Mass Spectrometry was a detector Quatromicro / Micromass from Waters,
a triple quadrupole with electron spray ionization (ESI). The parameters used were according to the
table:
Table IV. Parameters used in the MS analysis.
Instrument Parameters
Polarity ESI NEGATIVE
Capillary / kV 3.00
Cone / V 20.00
Extractor / V 3.00
RF Lens / V 0.50
Source Temperature / °C 140
Desolvation Temperature / °C
220
Cone Gas Flow / L h-1 60
Desolvation Gas Flow / L h-1
600
Infusion
Cycle time / s 10.100
Scan duration / s 10.000
Inter Scan Delay / s 0.100
Start and End Time / s 0.00 to 120.00
Ionization mode ESI NEGATIVE
or ESI POSITIVE
Data type Accurate Mass
Function type Scan
Mass range 20 to 1980
Syringe Pump Flow / µL min-1
20
- 28 -
4. Results and Discussion
4.1. Solvolysis Liquefaction
In order to have bio-oil for the electrochemical studies, three solvolysis liquefactions of cork
biomass were performed. The conditions of the liquefactions and their percentage of conversion, Eq.
[10], are presented in Table V:
Table V. Working conditions and conversion of the solvolysis liquefactions of milled cork biomass.
Liquefaction nº 1st. 2nd. 3rd.
Biomass / g 100 200 300
Solvent / g 200 400 600
Catalyst / g 6 12 18
Time / h 4 4 4
Solid Residue / g 33 64 98
Conversion / % 67 68 67
When compared the degree of conversion obtained in these liquefactions with similar ones found in
literature, such as Mateus et al. [33], the values are lower than expected. The reason might be related
to the ratio of biomass to solvent, as in the literature is usually 1:9, much higher than the ratio used in
this work. Another factor to have in consideration is the differences between cork dust or powder and
the grinded cork granules used during this work. The smaller cork particles combined with the higher
ratio of biomass to solvent may explain the higher conversion rates. Overall, the conversion values seem
to be consistent between the liquefactions produced during this work.
The bio-oils from olive stone and pinewood were produced with yields of around 60%, by a previous
master student colleague Sriram Hariharakrishnan [71] and gently provided for this study.
- 29 -
4.2. Bio-Oil Characterization
4.2.1. Physicochemical properties
The bio-oils characterization began by determining the values of density, viscosity, conductivity and
pH for each sample, which can be seen in Table VI. The value of viscosity was not properly determined
as the instrument was designed to measure the viscosity of very viscous materials, not measuring values
below the 0.1 Poise. It is also evident the low conductivity of all samples, which was predictable since
the media is an organic mixture of fragments from the depolymerization of cellulose and lignin.
Table VI. Physicochemical properties of the bio-oil samples, from the different biomasses.
Bio-Oils Density / g cm-3 Viscosity / P Conductivity / mS cm-1 pH
Cork 0.88 <0.1 0.5 x 10 -3 1.6
Pinewood 0.89 <0.1 1.0 x 10 -3 -0.5
Olive Stones 0.93 0.1 0.8 x 10 -3 0.4
Since the objective is to perform electrochemical studies, there is a need to increase the bio-oils
conductivity. Therefore, to increase the conductivity, it was added H2SO4 acid to the samples, see Table
VII. The value of the conductivity increased as expected, however the viscosity of the samples also
increased considerably with the addition of H2SO4. This increase of viscosity might suggest the
repolymerization of the bio-oil and may hinder the electrochemical studies. Comparing the different
samples, the cork bio-oil presents itself as the sample with the highest increase in conductivity and
lowest increase in viscosity. Figure 23 presents a graph of the increase of conductivity with the addition
of up to 3 M H2SO4 in a cork bio-oil sample.
Table VII. Conductivity and viscosity of the bio-oils with the addition of H2SO4 up to 3 M of concentration.
Bio-Oils H2SO4 / M Conductivity / mS cm-1 Viscosity / P
Cork
0 0.5 × 10-3 <0.1
1 1.23 0.3
3 5.34 1.5
Pinewood
0 0.8 × 10-3 <0.1
1 1.17 1.4
3 4.80 2.6
Olive Stones
0 1.0 × 10-3 0.1
1 0.74 11.0
3 1.85 19.1
- 30 -
Figure 23. The effect of the addition of H2SO4 in the conductivity of sample of cork bio-oil.
The same approach was tried with the addition of KOH to a stored sample of cork bio-oil, Table VIII.
Although the conductivity increased, the increase of viscosity was much higher than that observed
during the addition of acid to the cork bio-oil, with a viscosity of 9 P at 0.5 M KOH, thus the KOH addition
approach was abandoned.
Table VIII. Increase of conductivity with the addition of KOH in a sample of cork bio-oil.
KOH / M Conductivity / mS cm-1 Viscosity / P
0 1.8 0.8
0.05 2.4 ̶
0.10 2.8 ̶
0.15 3.4 ̶
0.30 3.7 ̶
0.50 4.9 9.0
- 31 -
4.3. Electrochemical Experiments
The two emulsions created for the electrochemical experiments consisted of a mixture of the cork
bio-oil with a 2 M H2SO4 aqueous solution, the emulsion EAc, and of a mixture with a 2 M KOH aqueous
solution, emulsion EAlk, according to Figure 20. In the case of the acidic emulsion it progressively
separated in several phases over a period of 12 hours, as seen in Figure 24 (A). On the other hand, in
(B), the emulsion EAlk did not form visible phase separation, instead, it contained a homogeneous
viscous residue at the bottom of the funnel. This lack of formation of visible phases in the alkali emulsion
was possibly due to the formation of phenolates, which are hydrophilic in nature; while in the acidic
emulsion the neutralization of such phenolates leads to a phase separation.
Figure 24. Emulsions of cork bio-oil with (A) a 2 M H2SO4 aqueous solution, EAc, with visible separation
of the phases of the emulsion after 12 hours and an (B) a 2M KOH aqueous solution, EAlk, with no visible
phases.
4.3.1. Cyclic Voltammetry
Cyclic voltammetry (CV) was used to assess the bio-oil samples anodic oxidation and cathodic
reduction at Pt electrodes. The CVs were performed in samples of cork, pinewood and olive stones bio-
oil with up to 3 M H2SO4 as well as in a mixture of cork bio-oil with an aqueous solution of 2 M H2SO4
and in a mixture of cork bio-oil with an aqueous solution of 2 M KOH.
The CVs for the samples of bio-oil of the different biomasses with 3M H2SO4 can be seen in Figure 25.
From the graphs, it is evident the low current densities as well as the lack of peaks across all samples,
indicating that no specific redox reaction was occurring at those potentials.
A B
- 32 -
Figure 25. CVs of the (A) cork, (B) pinewood and (C) olive stones bio-oils, performed at 50 mV s-1.
The CVs for the samples of cork bio-oil with 1 M and 3 M H2SO4 are present in Figure 26, where it is
observable an increase of current densities with the concentration of H2SO4, especially in the cathodic
zone. The current density for the sample with 3 M reaches maximum values of 1.1 mA cm-2 at 2 V, in
Figure 26 B, and -2.2 mA cm-2 at -2 V, in Figure 26 C. The increase of current densities in the cathodic
zone is expected as the addition of acid promotes the HER, the only reaction visible in this zone. The
maximum current density for each sample, in the CVs’ anodic and cathodic zones, can be seen in Table
IX.
Figure 27 shows the CVs of the pinewood bio-oil, pure and with concentrations of 1 M and 3 M H2SO4.
The CVs display similar behavior to the cork bio-oil CVs, with no visible peaks in the anodic zone, in
Figure 27 B, nor in the cathodic zone, in Figure 27 C. It displays an increase in the current densities
with the addition of H2SO4, with the highest current densities for the sample with 3 M being 1.74 mA
cm-2 at a potential of 2 V and -4.87 mA cm-2 at -2 V, (see Table IX), revealing an increase in the current
densities of over 3 orders of magnitude regarding the values for the pure pinewood bio-oil sample.
Figure 28 presents the CVs of the olive stones bio-oil sample, both pure and with concentrations of 1
M and 3 m H2SO4. The behavior is similar to the other bio-oils, having an increase in current densities
with the acid concentration. The maximum current densities in the 3 M H2SO4 sample, in Table IX, are
between 0.64 mA cm-2 for the potential of 2 V, in Figure 28 B, and -1.15 mA cm-2 for -2 V, in Figure 28
C.
Comparing the current densities between all bio-oil samples, visible in Table IX, one can ascertain that
the pinewood bio-oil samples show higher values across all concentrations of acid. At 3 M H2SO4, the
olive stones sample shows the lowest current densities for both anodic and cathodic zones. Only
considering the current densities shown in the CVs, the pinewood bio-oil shows better potential for the
electrolysis experiments. However, the cork bio-oil samples had a higher value of pH and conductivity,
while having a much smaller increase in viscosity with the addition of H2SO4.
- 33 -
Figure 26. CVs performed at 50 mV s-1 of (A) cork bio-oil samples, pure and with concentrations of 1 M
and 3 M H2SO4, as well as the respective (B) anodic zone and (C) cathodic zone.
Figure 27. The CVs of (A) pinewood bio-oil samples, pure and with concentrations of 1 M and 3 M
H2SO4, with (B) the anodic zone and (C) the cathodic zone. Performed at 50 mV s-1.
Figure 28. The CVs of (A) olive stones bio-oil samples, pure and with concentrations of 1 M and 3 M
H2SO4, as well as (B) and (C) the anodic and cathodic zones. Performed at 50 mV s-1.
- 34 -
Table IX. Current densities recorded in the CVs of the bio-oil samples at potentials of 2 V and -2 V.
Bio-Oils H2SO4 / M jE = 2 V / mA cm-2 jE = -2 V / mA cm-2
Cork
0 0.24 x 10-3 -0.27 x 10-3
1 0.33 -0.58
3 1.10 -2.23
Pinewood
0 1.09 x 10-3 -1.45 x 10-3
1 0.52 -0.79
3 1.74 -4.87
Olive Stones
0 0.99 x 10-3 -1.23 x 10-3
1 0.23 -0.34
3 0.64 -1.15
4.3.2. Linear Scan Voltammetry (LSV) and Tafel Analysis
The results obtained can be seen in Figure 29 where (A) is the LSVs of the cathodic zone,
performed at 50 mV s-1, for the olive stones, cork and pinewood bio-oils with 3 M H2SO4 and (B) is the
Tafel plot for the respective LSVs. The values of the OCP in the LSVs and the current density, j, at a
potential of -2 V are presented in Table X. The values of the linear equation, obtained from the linear
regression on the Tafel plot, Eq. [5], as well as the charge transfer coefficient, α, and the exchange
current density, j0, calculated from Eq. [6] and Eq. [7] respectively, are presented in Table XI. In Figure
29 (A) no reduction peak is visible in any of the LSVs, indicating that the only reduction reaction
happening in the cathode is the HER. Can also be seen that pinewood bio-oil sample has the highest
current densities at the same potential of all samples and olive stones having the lowest. From Figure
29 (B), the pinewood bio-oil has the smallest overpotential for comparable current densities, whereas
olive stones has the highest overpotential of the three samples. The Tafel slopes are between 0.59 V /
decade and 0.95 V / decade for pinewood and olive stones samples respectively.
Figure 29. The LSVs of (A) olive stones, cork and pinewood bio-oil samples with 3 M H2SO4, performed
at 50 mV s-1, with (B) Tafel plot for the respective samples with corresponding linear regression.
- 35 -
Table X. LSVs values of the OCP and of the current density, j, at a potential of -2 V.
Bio-Oils OCP / V jE=-2 V
/ mA cm-2
Cork 0.56 -2.23
Pinewood 0.24 -4.87
Olive Stones 0.67 -1.15
Table XI. The Tafel plot values of b, the Tafel Slope, and a, the y-interception of the linear regression
from the Tafel plots for each bio-oil sample, as well as the charge transfer coefficient, α, and the
exchange current density, j0, respectively.
Bio-Oils b / V dec-1 a / V α j0 / mA cm-2
Cork 0.59 1.25 0.10 7.4 x 10-3
Pinewood 0.56 0.73 0.11 49.4 x 10-3
Olive Stones 0.95 1.82 0.06 12.1 x 10-3
4.3.3. Chronoamperometry
The CAs for the cork bio-oil samples, both pure and with 3 M H2SO4 are present in Figure 30. For
the study of the behavior and stability of the samples, it was applied potentials 0.7 V and 1.3 V for the
anodic zone and -0.7 V and -1.3 V for the anodic zone, performed for 200 seconds.
In Figure 30 (A) and (B), the sample used was cork bio-oil and, due to the current densities in the order
of 10-4 mA cm-2, the CAs display some noise and are not well defined. Nonetheless, the behavior is the
expected one, with higher current densities for higher potentials and the current densities stabilize during
the 200 seconds run time. For the CAs in Figure 30 (C) and (D), it was used a sample of bio-oil with 3
M H2SO4. It shows the increase in the current densities, in comparison with the previous sample, while
displaying similar behavior, confirming that the addition of acid does not affect the behavior nor the
stability of the current densities.
For the samples of pinewood, the CAs present in Figure 31 (A) and (B), corresponds to the bio-oil
sample for the anodic and cathodic zones, respectively, together with (C) and (D), corresponding with
the sample with 3 M H2SO4, for the anodic and cathodic zones. The CAs are very similar between this
and the previous cork samples. The CA’s seem to be better defined for the anodic zone than for the
cathodic zone, where the fall of current densities with time is not as sharp.
For the olive stones bio-oil samples, the Figure 32 (A) and (B) shows the CAs for the anodic and
cathodic zones of the bio-oil, while Figure 32 (C) and (D) shows the CAs for the anodic and cathodic
zones for the bio-oil sample with 3 M H2SO4. The behavior of this bio-oil is similar to the other bio-oils
shown before, with (A) and (B) displaying low values of current density and poorly defined curves with
some noise. (C) and (D) show current densities about over 3 orders of magnitude superior to the ones
in the pure sample, also showing better defined curves, stabilizing at the 200 seconds of run time.
- 36 -
Figure 30. CAs for the pure cork bio-oil in the (A) anodic and (B) cathodic zones, as well as the CAs for
the cork bio-oil with 3 M H2SO4 in the (C) anodic and (D) cathodic zones, performed for 200 seconds.
Figure 31. CAs for the pinewood bio-oil in the (A) anodic and (B) cathodic zones as well as the CAs for
the pinewood bio-oil with 3 M H2SO4 for the (C) anodic and (D) cathodic zones, performed for 200
seconds.
- 37 -
Figure 32. CAs for the olive stones bio-oil in the (A) anodic and (B) cathodic zones as well as the CAs
for the olive stones bio-oil with 3 M H2SO4 for the (C) anodic and (D) cathodic zones, performed for 200
seconds.
The Figure 33, below, shows a comparison between the cork, pinewood and olive stones bio-oil
samples with 3 M H2SO4 in (A), the anodic zone and (B), the cathodic zone, at the same potential of
|0.9| V. It clearly shows the similar behavior between bio-oil samples, also shows the higher values of
current density of the pinewood bio-oil for the same potential. The fall in the current densities with time
in the anodic zone seems to be better defined than in the cathodic zone, where the characteristic curve
is barely visible.
Figure 33. Comparison between the CAs of the different bio-oils with 3 M H2SO4, at applied potential of
(A) 0.9 V for the anodic zone and (B) -0.9 V for the cathodic zone, performed for 200 seconds.
- 38 -
4.3.4. Electrolysis Experiments
The electrolyzes where performed for up to 24 hours in both a single compartment cell and a two-
compartment cell, as shown in Table III. As the low-precision power source used only shows currents
above 10 mA, it was not possible to record the electrolysis currents for the full time of the experiments.
Figure 34 presents the currents detected in the first 90 minutes of electrolysis experiment n1 of Table
III, of a cork bio-oil sample with 1.5 M H2SO4, in a single compartment cell with a couple of Ni plates of
22 cm2 of surface area as working electrodes. It shows a sharp decline of currents in the first few
minutes, stabilizing at values of 1.5 mA cm-2 and keeping those values for most of the registered time
until around 90 minutes of electrolysis where the current falls below the minimum value detected by the
power source.
Figure 34. Current densities observed in the first 90 minutes of electrolysis experiment n1 (see Table
III), the electrolysis of a cork bio-oil sample with 1.5 M H2SO4.
The electrolysis experiments n2 and n3 (Table III) with pinewood and olive stones, respectively,
followed the same procedure used on electrolysis experiment n1, however, the currents produced were
below the detection range of the power source, which is 10 mA. The same behavior was shown in the
electrolysis experiment n4, of the emulsion EAc, the currents produced were below the detection range
of the power source.
The currents observed for the first 25 minutes of the electrolysis experiment n5, the emulsion of cork
bio-oil with a 2 M KOH aqueous solution, emulsion EAlk (see diagram in Figure 20), performed with
continuous mechanical agitation in the single compartment cell, can be seen in Figure 35. The currents
stabilized in the first 25 minutes and maintained the current densities of around 0.9 mA cm-2 for the
entire duration of the 24 hours electrolysis.
- 39 -
Figure 35. Current densities observed in the first 25 minutes of electrolysis experiment n5 (see Table
III), the electrolysis of an emulsion of cork bio-oil sample with 2 M KOH aqueous solution in a single
compartment cell.
The two electrolysis experiments n6 and n7 of the Table III, with cork bio-oil sample with 2 M H2SO4 as
the anodic electrolyte in the two-compartment cell were performed for 14 hours. In these electrolysis
experiments n6 and n7 it was used a 2 M H2SO4 cork bio-oil sample and a 2 M H2SO4 aqueous solution
as electrolytes in the cathodic compartment, respectively, with an industrial membrane separating the
two compartments. Just like several electrolysis experiments in the single compartment cell, these
experiments did not produce currents above the minimum value detectable by the power source.
The electrolysis experiment n8 from Table III, used emulsion EAc, as electrolyte in the cathodic side and
emulsion EAlk as electrolyte in the anodic cell was performed for 24 hours, with continuous mechanical
agitation in both compartments, and the currents detected in the first 10 minutes can be seen in Figure
36. The currents stabilized at values around 2.2 mA cm-2 in the first 10 minutes of electrolysis and
maintained that values for the entire duration.
- 40 -
Figure 36. Current densities observed in the first 10 minutes of electrolysis experiment n8 (see Table
III), the electrolysis of an acidic emulsion EAc as electrolyte in the cathodic side and an alkali emulsion
EAlk as electrolyte in the anodic cell, performed for 24 hours.
The summary of the value of the current, at the end of each electrolysis experiment can be seen on
Table XII. From the table, it is evident the higher currents obtained during the electrolysis experiment
n8. It is also visible the low currents for all electrolysis experiments performed with the addition of H2SO4
to the samples, where the currents are below the detection range of the power source.
The samples subjected to electrolysis were then analyzed by ATR-FTIR and MS to determine possible
changes in their composition. By the analysis of the currents during electrolysis, it would be expected
for the samples of the electrolysis experiments n5 and n8 to show higher degree of difference between
their initial and final compositions.
Table XII. Resume of the values of jtf, the current densities detected at the end of each electrolysis
08102018_CORK_MIX_ACET_AMON_ESINEG_01 8 (1.348) Cm (2:11) Scan ES- 5.00e5
A
B
C
A
B
C
C
Figure 55. The MS with negative ESI of (A) sample of cork bio-oil, (B) alkali emulsion EAlk, (C) emulsion viscous residue EAlk-Res, (D) emulsion phase EAlk’ and (E) emulsion phase EAlk-Res’.