Top Banner
1 of 8 © Boardworks Ltd 2009
8
Welcome message from author
This document is posted to help you gain knowledge. Please leave a comment to let me know what you think about it! Share it to your friends and learn new things together.
Transcript
Page 1: Energetics part 2   calorimetry

1 of 8 © Boardworks Ltd 2009

Page 2: Energetics part 2   calorimetry

2 of 8 © Boardworks Ltd 2009

Enthalpy of combustion experiment

Page 3: Energetics part 2   calorimetry

3 of 8 © Boardworks Ltd 2009

Enthalpy of neutralization experiment

Page 4: Energetics part 2   calorimetry

4 of 8 © Boardworks Ltd 2009

Using experimental results

Page 5: Energetics part 2   calorimetry

5 of 8 © Boardworks Ltd 2009

Calorimetry calculations

Enthalpy change can be calculated using the following equation:

q = mc∆T

q = enthalpy change in joules

To work out the enthalpy of neutralization, the density and specific heat capacities of the acid and base used are taken to be the same as for pure water.

∆T = change of temperature in Kelvin.

c = specific heat capacity in joules per Kelvin per gram (4.18 JK-1g-1 for water)

m = mass of substance being heated (often water) in grams

Page 6: Energetics part 2   calorimetry

6 of 8 © Boardworks Ltd 2009

Calorimetry calculation examples

Page 7: Energetics part 2   calorimetry

7 of 8 © Boardworks Ltd 2009

Calorimetry calculation problems

Page 8: Energetics part 2   calorimetry

8 of 36 © Boardworks Ltd 20098 of 36 © Boardworks Ltd 20098 of 8 © Boardworks Ltd 2009

The bomb calorimeter