Combined Past Paper Questions on Stoiciometry

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7 Chemists use the concept of the mole to calculate the amounts of chemicals involved in a

reaction.

(a) Define mole.

[1]

(b) 3.0g of magnesium was added to 12.0g of ethanoic acid.

Mg + 2CH3COOH → (CH

3COO)

2Mg + H

2

The mass of one mole of Mg is 24g.

The mass of one mole of CH3COOH is 60 g.

(i) Which one, magnesium or ethanoic acid, is in excess? You must show your

reasoning.

[3]

(ii) How many moles of hydrogen were formed?

[1]

(iii) Calculate the volume of hydrogen formed, measured at r.t.p.

[2]

(c) In an experiment, 25.0cm3

of aqueous sodium hydroxide, 0.4mol / dm3

, was neutralised

by 20.0cm3

of aqueous oxalic acid, H2C

2O

4.

2NaOH + H2C

2O

4→ Na

2C

2O

4 +2H

2O

Calculate the concentration of the oxalic acid in mol / dm3

.

(i) Calculate the number of moles of NaOH in 25.0cm3

of 0.4 mol / dm3

solution.

[1]

(ii) Use your answer to (i) and the mole ratio in the equation to find out the number of

moles of H2C

2O

4 in 20 cm

3

of solution.

[1]

(iii) Calculate the concentration, mol / dm3

, of the aqueous oxalic acid.

[2]

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(iii) Draw a diagram to show the arrangement of the valency electrons in one molecule of the covalent compound hydrogen sulphide.

Use o to represent an electron from a sulphur atom. Use x to represent an electron from a hydrogen atom. [2] (c) Sulphuric acid is manufactured by the Contact Process. Sulphur dioxide is oxidised to

sulphur trioxide by oxygen.

2SO2 + O2 2SO3 (i) Name the catalyst used in this reaction.

[1]

(ii) What temperature is used for this reaction?

[1]

(iii) Describe how sulphur trioxide is changed into sulphuric acid.

[2]

(d) Gypsum is hydrated calcium sulphate, CaSO4.xH2O. It contains 20.9% water by mass.

Calculate x.

Mr: CaSO4, 136; H2O, 18.

79.1 g of CaSO4 = moles

20.9 g of H2O = moles

x = [3]

15

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© UCLES 2006 0620/03/M/J/06

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(c) Alkenes are more reactive than alkanes and are used to make a range of organic chemicals. Propene, CH3–CH=CH2, is made by cracking. Give the structural formula of the addition product when propene reacts with the following.

(i) water [1] (ii) bromine [1] (d) Propene reacts with hydrogen iodide to form 2 - iodopropane.

CH3−CH=CH2 + HI CH3−CHI−CH3

1.4 g of propene produced 4.0 g of 2 - iodopropane. Calculate the percentage yield.

moles of CH3–CH=CH2 reacted =

maximum moles of CH3–CHI–CH3 that could be formed =

mass of one mole of CH3–CHI–CH3 = 170 g

maximum mass of 2 - iodopropane that could be formed =

percentage yield % [4]

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(d) A better way of measuring the degree of unsaturation is to find the iodine number of the unsaturated compound. This is the mass of iodine that reacts with all the double bonds in 100 g of the fat.

Use the following information to calculate the number of double bonds in one molecule

of the fat. Mass of one mole of the fat is 884 g.

One mole of I2 reacts with one mole C C.

The iodine number of the fat is 86.2 g. Complete the following calculation.

100 g of fat reacts with 86.2 g of iodine.

884 g of fat reacts with g of iodine.

One mole of fat reacts with moles of iodine molecules.

Number of double bonds in one molecule of fat is [3]

[Total:14]

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7 Crystals of sodium sulphate-10-water, Na2SO4.10H2O, are prepared by titration.

conical flask

burette filled with

sulphuric acid

25.0 cm3 of sodium hydroxide(aq)

concentration 2.24 mol / dm3

(a) 25.0 cm3 of aqueous sodium hydroxide is pipetted into a conical flask. A few drops of an indicator are added. Using a burette, dilute sulphuric acid is slowly

added until the indicator just changes colour. The volume of acid needed to neutralise the alkali is noted.

Suggest how you would continue the experiment to obtain pure, dry crystals of sodium sulphate-10-water.

[4]

(b) Using 25.0 cm3 of aqueous sodium hydroxide, 2.24 mol / dm3, 3.86 g of crystals were obtained. Calculate the percentage yield.

2NaOH + H2SO4 Na2SO4 + 2H2O

Na2SO4 + 10H2O Na2SO4.10H2O

Number of moles of NaOH used =

Maximum number of moles of Na2SO4.10H2O that could be formed =

Mass of one mole of Na2SO4.10H2O = 322 g

Maximum yield of sodium sulphate-10-water = g

Percentage yield = % [4]

[Total: 8]

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9 Quantities of chemicals, expressed in moles, can be used to find the formula of a compound, to establish an equation and to determine reacting masses.

(a) A compound contains 72% magnesium and 28% nitrogen. What is its empirical

formula?

[2]

(b) A compound contains only aluminium and carbon. 0.03 moles of this compound reacted

with excess water to form 0.12 moles of Al(OH)3 and 0.09 moles of CH4. Write a balanced equation for this reaction.

[2]

(c) 0.07 moles of silicon reacts with 25 g of bromine.

Si + 2Br2 SiBr4 (i) Which one is the limiting reagent? Explain your choice.

[3]

(ii) How many moles of SiBr4 are formed?

[1]

[Total: 8]

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(e) The titanium ore contains 36.8% iron, 31.6% titanium and the remainder is oxygen.

(i) Determine the percentage of oxygen in this titanium compound.

percentage of oxygen = ........................................................................... % [1]

(ii) Calculate the number of moles of atoms for each element. The number of moles of Fe is shown as an example. number of moles of Fe = 36.8 / 56 = 0.66

number of moles of Ti = ...........................................................................................

number of moles of O = ..................................................................................... [1]

(iii) What is the simplest ratio for the moles of atoms?

Fe : Ti : O

............. ............. .............[1]

(iv) What is the formula of this titanium compound?

.............................................................................................................................. [1]

[Total: 10]

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(c) A 5.00 g sample of impure lead(II) nitrate was heated. The volume of oxygen formed was 0.16 dm3 measured at r.t.p. The impurities did not decompose.

Calculate the percentage of lead(II) nitrate in the sample.

2Pb(NO3)2 → 2PbO + 4NO2 + O2

Number of moles of O2 formed = .......................................

Number of moles of Pb(NO3)2 in the sample = .......................................

Mass of one mole of Pb(NO3)2 = 331 g

Mass of lead(II) nitrate in the sample = ....................................... g

Percentage of lead(II) nitrate in sample = ..................................... [4]

[Total: 10]

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(iii) Two salts of phosphorus acid are its sodium salt, which is soluble in water, and its calcium salt which is insoluble in water. Suggest a method of preparation for each of these salts from aqueous phosphorus acid. Specify any other reagent needed and briefl y outline the method.

sodium salt ................................................................................................................

....................................................................................................................................

....................................................................................................................................

.............................................................................................................................. [2]

calcium salt ................................................................................................................

....................................................................................................................................

....................................................................................................................................

.............................................................................................................................. [2]

[Total: 10]

8 Hydrocarbons are compounds which contain only carbon and hydrogen.

(a) 20 cm3 of a gaseous hydrocarbon was burned in 120 cm3 of oxygen, which is in excess. After cooling, the volume of the gases remaining was 90 cm3. Aqueous sodium hydroxide was added to remove carbon dioxide, 30 cm3 of oxygen remained. All volumes were measured at r.t.p..

(i) Explain why it is essential to use excess oxygen.

....................................................................................................................................

.............................................................................................................................. [2]

(ii) Carbon dioxide is slightly soluble in water. Why does it dissolve readily in the alkali, sodium hydroxide?

.............................................................................................................................. [1]

(iii) Complete the following.

volume of gaseous hydrocarbon = ...............cm3

volume of oxygen used = .............cm3

volume of carbon dioxide formed = .............cm3 [2]

(iv) Use the above volume ratio to fi nd the mole ratio in the equation below and hence fi nd the formula of the hydrocarbon.

........CxHy(g) + ........O2(g) → ........CO2(g) + ........H2O(l)

hydrocarbon formula = ................................................ [2]

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(b) A sample of rust had the following composition:

51.85 g of iron 22.22 g of oxygen 16.67 g of water.

Calculate the following and then write the formula for this sample of rust.

number of moles of iron atoms, Fe = ................... [1]

number of moles of oxygen atoms, O = ................... [1]

number of moles of water molecules, H2O = ................... [1]

simplest mole ratio Fe : O : H2O is .......... : .......... : ..........

formula for this sample of rust is ................... [1]

[Total: 12]

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(e) 0.01 moles of an alkene needed 2.4 g of oxygen for complete combustion. 2.2 g of carbon dioxide were formed. Determine the following mole ratio.

moles of alkene : moles of O2 : moles of CO2

From this ratio determine the formula of the alkene.

..................................................................................................................................... [3]

Write an equation for the complete combustion of this alkene.

..................................................................................................................................... [1]

[Total: 13]

8 Ethylamine, CH3–CH2–NH2, is a base which has similar properties to ammonia.

(a) In aqueous ethylamine, there is the following equilibrium.

CH3–CH2–NH2 + H2O CH3–CH2–NH3+ + OH–

Explain why water is behaving as an acid in this reaction.

..................................................................................................................................... [1]

(b) Given aqueous solutions of ethylamine and sodium hydroxide, describe how you could show that ethylamine is a weak base like ammonia and not a strong base like sodium hydroxide.

...........................................................................................................................................

...........................................................................................................................................

..................................................................................................................................... [3]

(c) Ethylamine, like ammonia, reacts with acids to form salts.

CH3–CH2–NH2 + HCl → CH3–CH2–NH3Cl

ethylammonium chloride

Suggest how you could displace ethylamine from the salt, ethylammonium chloride.

...........................................................................................................................................

..................................................................................................................................... [2]

6

0620/3/O/N/02

(e) Draw a diagram that shows the arrangement of the valency electrons in the ionic compound sodium phosphide.

Use o to represent an electron from sodium.Use x to represent an electron from phosphorus. [3]

(f) Sodium reacts with sulphur to form sodium sulphide.

2Na + S → Na2S

An 11.5 g sample of sodium is reacted with 10 g of sulphur. All of the sodium reacted butthere was an excess of sulphur. Calculate the mass of sulphur left unreacted.

(i) Number of moles of sodium atoms reacted = .....................[2 moles of Na react with 1 mole of S]

(ii) Number of moles of sulphur atoms that reacted = ..................

(iii) Mass of sulphur reacted = ...................g

(iv) Mass of sulphur left unreacted = .................g [4]

4 For over 5000 years copper has been obtained by the reduction of its ores. More recently themetal has been purified by electrolysis.

(a) Copper is used to make alloys.

(i) Give two other uses of copper.

...............................................................................................................................[2]

(ii) Alloys have similar structures to pure metals. Give a labelled diagram that showsthe structure of a typical alloy, such as brass.

[3]

ForExaminer’s

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0620/03/O/N/03

5 Sulphur dioxide, SO2, and sulphur trioxide, SO3, are the two oxides of sulphur.

(a) Sulphur dioxide can kill bacteria and has bleaching properties. Give a use of sulphurdioxide that depends on each of these properties.

(i) ability to kill bacteria .............................................................................................[1]

(ii) bleaching properties .............................................................................................[1]

(b) Sulphur trioxide can be made from sulphur dioxide.

(i) Why is this reaction important industrially?

...............................................................................................................................[1]

(ii) Complete the word equation.

sulphur dioxide + ……………….……………………… → sulphur trioxide [1]

(iii) What are the conditions for this reaction?

...................................................................................................................................

...............................................................................................................................[2]

(c) Sulphur dioxide is easily oxidised in the presence of water.

SO2 + 2H2O – 2e– → SO42– + 4H+

(i) What colour change would be observed when an excess of aqueous sulphurdioxide is added to an acidic solution of potassium manganate(VII)?

...............................................................................................................................[2]

(ii) To aqueous sulphur dioxide, acidified barium chloride solution is added. The mixtureremains clear. When bromine is added, a thick white precipitate forms. What is thewhite precipitate? Explain why it forms.

...................................................................................................................................

...............................................................................................................................[3]

(d) Sulphur dioxide reacts with chlorine in an addition reaction to form sulphuryl chloride.

SO2 + Cl2 → SO2Cl2

8.0 g of sulphur dioxide was mixed with 14.2 g of chlorine. The mass of one mole ofSO2Cl2 is 135 g.

Calculate the mass of sulphuryl chloride formed by this mixture.

Calculate the number of moles of SO2 in the mixture = ………………

Calculate the number of moles of Cl2 in the mixture = ………………

Which reagent was not in excess? ………………………….

How many moles of SO2Cl2 were formed = ……………….

Calculate the mass of sulphuryl chloride formed = …………. g [5]

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12

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7 (a) (i) Write a symbol equation for the action of heat on zinc hydroxide.

[2]

(ii) Describe what happens when solid sodium hydroxide is heated strongly.

[1]

(b) What would be observed when copper(II) nitrate is heated?

[3]

(c) Iron(III) sulphate decomposes when heated. Calculate the mass of iron(III) oxide

formed and the volume of sulphur trioxide produced when 10.0 g of iron(III) sulphate was heated.

Mass of one mole of Fe2(SO4)3 is 400 g.

Fe2(SO4)3 (s) Fe2O3 (s) + 3SO3 (g)

Number of moles of Fe2(SO4)3 =

Number of moles of Fe2O3 formed =

Mass of iron(III) oxide formed = g

Number of moles of SO3 produced =

Volume of sulphur trioxide at r.t.p. = dm3 [5]

11

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6 (a) The following method is used to make crystals of hydrated nickel sulphate. An excess of nickel carbonate, 12.0 g, was added to 40 cm3 of sulphuric acid, 2.0

mol/dm3. The unreacted nickel carbonate was filtered off and the filtrate evaporated to obtain the crystals.

NiCO3 + H2SO4 NiSO4 + CO2 + H2O

NiSO4 + 7H2O NiSO4.7H2O Mass of one mole of NiSO4.7H2O = 281 g Mass of one mole of NiCO3 = 119 g (i) Calculate the mass of unreacted nickel carbonate.

Number of moles of H2SO4 in 40 cm3 of 2.0 mol/dm3 acid = 0.08

Number of moles of NiCO3 reacted =

Mass of nickel carbonate reacted = g

Mass of unreacted nickel carbonate = g [3]

(ii) The experiment produced 10.4 g of hydrated nickel sulphate. Calculate the

percentage yield.

The maximum number of moles of NiSO4 .7H2O that could be formed =

The maximum mass of NiSO4 .7H2O that could be formed = g

The percentage yield = % [3]

(b) In the above method, a soluble salt was prepared by neutralising an acid with an

insoluble base. Other salts have to be made by different methods. (i) Give a brief description of how the soluble salt, rubidium sulphate could be made

from the soluble base, rubidium hydroxide.

[3]

8

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6 An ore of copper is the mineral, chalcopyrite. This is a mixed sulphide of iron and copper. (a) Analysis of a sample of this ore shows that 13.80 g of the ore contained 4.80 g of

copper, 4.20 g of iron and the rest sulphur. Complete the table and calculate the empirical formula of chalcopyrite.

copper iron sulphur

composition by mass / g 4.80 4.20

number of moles of atoms

simplest mole ratio of atoms

[3] The empirical formula is

[1]

(b) Impure copper is extracted from the ore. This copper is refined by electrolysis. (i) Name; the material used for the positive electrode (anode),

the material used for the negative electrode (cathode),

a suitable electrolyte.

[3]

(ii) Write an ionic equation for the reaction at the negative electrode.

[1]

(iii) One use of this pure copper is electrical conductors, another is to make alloys.

Name the metal that is alloyed with copper to make brass.

[1]

12

© UCLES 2007 0620/03/O/N/07

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(b) An alternative method of measuring the rate of this reaction would be to measure the volume of carbon dioxide produced at regular intervals.

(i) Sketch this graph

volume

time [2] (ii) One piece of marble, 0.3 g, was added to 5 cm3 of hydrochloric acid, concentration

1.00 mol / dm3. Which reagent is in excess? Give a reason for your choice.

mass of one mole of CaCO3 = 100 g

number of moles of CaCO3 =

number of moles of HCl =

reagent in excess is

reason [4]

(iii) Use your answer to (ii) to calculate the maximum volume of carbon dioxide

produced measured at r.t.p.

[1]

[Total: 13]

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© UCLES 2008 0620/31/O/N/08

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3 Steel is an alloy made from impure iron. (a) Both iron and steel rust. The formula for rust is Fe2O3.2H2O. It is hydrated iron(III) oxide. (i) Name the two substances that must be present for rusting to occur.

[2]

(ii) Painting and coating with grease are two methods of preventing iron or steel from

rusting. Give two other methods.

[2]

(b) (i) Name a reagent that can reduce iron(III) oxide to iron.

[1]

(ii) Write a symbol equation for the reduction of iron(III) oxide, Fe2O3, to iron.

[2]

(c) (i) Calculate the mass of one mole of Fe2O3.2H2O.

[1]

(ii) Use your answer to (i) to calculate the percentage of iron in rust.

[2]

(d) Iron from the blast furnace is impure. Two of the impurities are carbon and silicon.

These are removed by blowing oxygen through the molten iron and adding calcium oxide.

(i) Explain how the addition of oxygen removes carbon.

[1]

(ii) Explain how the addition of oxygen and calcium oxide removes silicon.

[2]

[Total: 13]

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(iii) The following is a redox reaction.

Mn + Sn2+ Mn2+ + Sn Indicate on the equation the change which is oxidation. Give a reason for your choice.

[2]

(iv) Explain why experiments of this type cannot be used to find the position of

aluminium in the reactivity series.

[2]

(b) Potassium and calcium are very reactive metals at the top of the series. Because their

ions have different charges, K+ and Ca2+, their compounds behave differently when heated.

(i) Explain why the ions have different charges.

[2]

(ii) Their hydroxides are heated. If the compound decomposes, complete the word equation. If it does not decompose, write “no reaction”.

Potassium hydroxide

Calcium hydroxide [2]

(iii) Complete the equations for the decomposition of their nitrates.

2KNO3 +

2Ca(NO3)2 + + [4]

[Total: 17]

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(b) Sulfuric acid was first made in the Middle East by heating the mineral, green vitriol, FeSO4.7H2O. The gases formed were cooled.

FeSO4.7H2O(s) → FeSO4(s) + 7H2O(g) green crystals yellow powder

2FeSO4(s) → Fe2O3(s) + SO2(g) + SO3(g)

On cooling

SO3 + H2O → H2SO4 sulfuric acid

SO2 + H2O → H2SO3 sulfurous acid (i) How could you show that the first reaction is reversible?

[2]

(ii) Sulfurous acid is a reductant. What would you see when acidified potassium

manganate(VII) is added to a solution containing this acid?

[2]

(iii) Suggest an explanation why sulfurous acid in contact with air changes into sulfuric

acid.

[1]

(c) 9.12 g of anhydrous iron(II) sulfate was heated. Calculate the mass of iron(III) oxide formed and the volume of sulfur trioxide, at r.t.p., formed.

2FeSO4(s) → Fe2O3(s) + SO2(g) + SO3(g)

mass of one mole of FeSO4 = 152 g

number of moles of FeSO4 used =

number of moles of Fe2O3 formed =

mass of one mole of Fe2O3 = g

mass of iron(III) oxide formed = g

number of moles of SO3 formed =

volume of sulfur trioxide formed = dm3

[6] [Total: 16]

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(b) 6.0 g of cobalt(II) carbonate was added to 40 cm3 of hydrochloric acid, concentration2.0 mol / dm3. Calculate the maximum yield of cobalt(II) chloride-6-water and show that the cobalt(II) carbonate was in excess.

CoCO3 + 2HCl → CoCl 2 + CO2 + H2O

CoCl 2 + 6H2O → CoCl 2.6H2O

Maximum yield

Number of moles of HCl used = .........................

Number of moles of CoCl 2 formed = .........................

Number of moles of CoCl 2.6H2O formed = .........................

Mass of one mole of CoCl 2.6H2O = 238 g

Maximum yield of CoCl 2.6H2O = ......................... g [4]

To show that cobalt(II) carbonate is in excess

Number of moles of HCl used = ......................... (use value from above)

Mass of one mole of CoCO3 = 119 g

Number of moles of CoCO3 in 6.0 g of cobalt(II) carbonate = ......................... [1]

Explain why cobalt(II) carbonate is in excess .................................................................

..................................................................................................................................... [1]

[Total: 10]

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(d) 20.0 cm3 of sulfuric acid, concentration 0.30 mol / dm3, was added to 40 cm3 of sodium hydroxide, concentration 0.20 mol / dm3.

2NaOH + H2SO4 → Na2SO4 + 2H2O

(i) How many moles of H2SO4 were added? .............................. [1]

(ii) How many moles of NaOH were used? .............................. [1]

(iii) Which reagent is in excess? Give a reason for your choice.

reagent in excess ............................................................................................... [1]

reason .......................................................................................................................

.............................................................................................................................. [1]

(iv) Is the pH of the fi nal mixture less than 7, equal to 7 or more than 7?

.............................................................................................................................. [1]

[Total: 15]

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7 Some hydroxides, nitrates and carbonates decompose when heated.

(a) (i) Name a metal hydroxide which does not decompose when heated.

.............................................................................................................................. [1]

(ii) Write the equation for the thermal decomposition of copper(II) hydroxide.

.............................................................................................................................. [2]

(iii) Suggest why these two hydroxides behave differently.

.............................................................................................................................. [1]

(b) (i) Metal nitrates, except those of the Group 1 metals, form three products when heated. Name the products formed when zinc nitrate is heated.

....................................................................................................................................

.............................................................................................................................. [2]

(ii) Write the equation for the thermal decomposition of potassium nitrate.

.............................................................................................................................. [2]

(c) There are three possible equations for the thermal decomposition of sodium hydrogencarbonate.

2NaHCO3(s) → Na2O(s) + 2CO2(g) + H2O(g) equation 1 NaHCO3(s) → NaOH(s) + CO2(g) equation 2 2NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(g) equation 3

The following experiment was carried out to determine which one of the above is the correct equation.

A known mass of sodium hydrogencarbonate was heated for ten minutes. It was then allowed to cool and weighed.

Results Mass of sodium hydrogencarbonate = 3.36 g Mass of the residue = 2.12 g

Calculation Mr for NaHCO3 = 84 g; Mr for Na2O = 62 g; Mr for NaOH = 40 g Mr for Na2CO3 = 106 g

(i) Number of moles of NaHCO3 used = ............... [1]

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(ii) If residue is Na2O, number of moles of Na2O = ...............

If residue is NaOH, number of moles of NaOH = ...............

If residue is Na2CO3, number of moles of Na2CO3 = ............... [2]

(iii) Use the number of moles calculated in (i) and (ii) to decide which one of the three equations is correct. Explain your choice.

....................................................................................................................................

....................................................................................................................................

.............................................................................................................................. [2]

[Total: 13]

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(c) Insoluble salts are made by precipitation. An equation for the preparation of barium sulfate is given below.

BaCl 2(aq) + MgSO4(aq) → BaSO4(s) + MgCl 2(aq)

This reaction can be used to fi nd x in the formula for hydrated magnesium sulfateMgSO4.xH2O.

A known mass of hydrated magnesium sulfate, MgSO4.xH2O, was dissolved in water. Excess aqueous barium chloride was added. The precipitate of barium sulfate was fi ltered, washed and dried. Finally it was weighed.

Mass of hydrated magnesium sulfate = 1.476 g

Mass of barium sulfate formed = 1.398 g

The mass of one mole of BaSO4 = 233 g

The number of moles of BaSO4 formed = ............... [1]

The number of moles of MgSO4.xH2O = ............... [1]

The mass of one mole of MgSO4.xH2O = ............... g [1]

The mass of one mole of MgSO4 = 120 g

The mass of xH2O in one mole of MgSO4.xH2O = ............... [1]

x = ............... [1]

[Total: 15]

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(b) Strontium chloride-6-water can be made from the insoluble compound, strontium carbonate, by the following reactions.

SrCO3(s) + 2HCl (aq) → SrCl 2(aq) + CO2(g) + H2O(l)

SrCl 2 (aq) + 6H2O(l) → SrCl 2.6H2O(s)

The following method was used to prepare the crystals.

1 Add excess strontium carbonate to hot hydrochloric acid. 2 Filter the resulting mixture. 3 Partially evaporate the filtrate and allow to cool. 4 Filter off the crystals of SrCl 2.6H2O. 5 Dry the crystals between filter papers.

(i) How would you know when excess strontium carbonate had been added in step 1?

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.............................................................................................................................. [1]

(ii) Why is it necessary to fi lter the mixture in step 2?

.............................................................................................................................. [1]

(iii) In step 3, why partially evaporate the fi ltrate rather than evaporate to dryness?

.............................................................................................................................. [1]

(c) In the above experiment, 50.0 cm3 of hydrochloric acid of concentration 2.0 mol / dm3 was used. 6.4 g of SrCl 2.6H2O was made.

Calculate the percentage yield.

number of moles of HCl used = ............................

number of moles of SrCl 2.6H2O which could be formed = ............................

mass of one mole of SrCl 2.6H2O is 267 g

theoretical yield of SrCl 2.6H2O = ............................g

percentage yield = ............................% [4]

[Total: 15]

8

0620/32/O/N/12© UCLES 2012

ForExaminer’s

Use

5 The food additive E220 is sulfur dioxide. It is a preservative for a variety of foods and drinks.

(a) State two other uses of sulfur dioxide.

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..................................................................................................................................... [2]

(b) How is sulfur dioxide manufactured?

...........................................................................................................................................

..................................................................................................................................... [2]

(c) Sulfur dioxide is a reductant (reducing agent). Describe what you would see when aqueous sulfur dioxide is added to acidifi ed potassium manganate(VII).

...........................................................................................................................................

..................................................................................................................................... [2]

(d) Sulfur dioxide can also be made by the reaction between a sulfi te and an acid.

Na2SO3 + 2HCl → 2NaCl + SO2 + H2O

Excess hydrochloric acid was added to 3.15 g of sodium sulfi te. Calculate the maximum volume, measured at r.t.p., of sulfur dioxide which could be formed.

The mass of one mole of Na2SO3 is 126 g.

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...........................................................................................................................................

..................................................................................................................................... [3]

[Total: 9]