Measurement of an Enthalpy Change (Oxford AQA International A Level Chemistry)
Revision Note
Written by: Alexandra Brennan
Reviewed by: Stewart Hird
Required Practical 2: Measuring Enthalpy Change
Objective
To determine the enthalpy change for the conversion of anhydrous copper(II) sulfate into hydrated copper(II) sulfate, ΔH3
This enthalpy change cannot be measured directly but can be calculated from:
The enthalpy change for the conversion of anhydrous copper sulfate to copper sulfate solution, ΔH1
The enthalpy change for the conversion of hydrate copper sulfate to copper sulfate solution, ΔH2
Apparatus
Hydrated copper(II) sulfate crystals
Anhydrous copper(II) sulfate powder
Polystyrene cups with lids
250 cm3 for holding polystyrene cup
Stand and clamp
Thermometer
25 cm3 measuring cylinders x 2
Weighing bottles x 2
Stopwatch
Graph paper
Stirrer
Distilled water
Digital balance
Method
Experiment 1: Determining ΔH1
Weigh out between 3.90 g and 4.10 g of anhydrous copper(II) sulfate in a weighing bottle and record the mass
Measure 25 cm3 of deionised water into a polystyrene cup using a measuring cylinder
Record its temperature at the beginning (t=0)
Start the timer and record the temperature every minute for a further three minutes
At the fourth minute, add the powdered anhydrous copper(II) sulfate rapidly to the polystyrene cup and continue to stir, but do not record the temperature.
At the fifth minute and for every minute up to 15 minutes, stir and record the temperature of the solution in the polystyrene cup.
Experiment 2: Determining ΔH2
Weigh out between 6.20 g and 6.30 g of hydrated copper(II) sulfate in a weighing bottle and record the mass
Measure 24 cm3 of deionised water into a polystyrene cup using a measuring cylinder
Record its temperature at the beginning (t=0)
Start the timer and record the temperature every minute for a further three minutes
At the fourth minute, add the powdered hydrated copper(II) sulfate rapidly to the polystyrene cup and continue to stir, but do not record the temperature.
At the fifth minute and for every minute up to 15 minutes, stir and record the temperature of the solution in the polystyrene cup.
How to set up your equipment
Practical Tip
Be careful not to get the anhydrous copper(II) on your skin as it can cause irritation.
Results
Record your results in a table like this:
Temperature / oC | Experiment 1 | Experiment 2 |
---|---|---|
0 | ||
1 | ||
2 | ||
3 | ||
4 | x | x |
5 | ||
6 | ||
7 | ||
8 | ||
9 | ||
10 | ||
11 | ||
12 | ||
13 | ||
14 | ||
15 |
The temperature is not recorded at minute 4 as this is when you have added the hydrated / anhydrous copper(II) sulfate.
Evaluation
For each set of results:
Plot a graph of temperature (on the y-axis) against time (on the x-axis)
Draw two separate best fit lines; one, which joins the points before the addition of hydrated / anhydrous copper(II) sulfate, and one which joins the points after the addition
Extrapolate both lines to the fourth minute
Use your graph to determine the temperature change at the fourth minute
Use q = m x c x ΔT and ΔH = q/ n to determine ΔH1 and ΔH2
Determine the enthalpy change for ΔH3 using:
ΔH3 = ΔH1 – ΔH2
Worked Example
A student obtained the data in Table 1 by carrying out the methods above.
They added 4.94 g anhydrous copper(II) sulfate in experiment 1.
They added 7.72 g hydrated copper(II) sulfate in experiment 2.
Table 1
Temperature / oC | Experiment 1 | Experiment 2 |
---|---|---|
0 | 19.8 | 19.6 |
1 | 19.8 | 19.8 |
2 | 19.8 | 19.8 |
3 | 19.8 | 19.8 |
4 | x | x |
5 | 27.8 | 18.2 |
6 | 27.7 | 18.2 |
7 | 27.6 | 18.2 |
8 | 27.6 | 18.2 |
9 | 27.5 | 18.2 |
10 | 27.5 | 18.2 |
11 | 27.4 | 18.2 |
12 | 27.3 | 18.2 |
13 | 27.2 | 18.2 |
14 | 27.0 | 18.2 |
15 | 26.8 | 18.2 |
Question
Plot a graph of each set of results to determine the temperature change for each reaction
Calculate the enthalpy change for each reaction, ΔH
Calculate the enthalpy change, in kJ mol –1 for the hydration of copper(II) sulfate.
The specific heat capacity of water is 4.2 J/kg°C.
Answer:
The graphs for each set of results and temperature changes are:
Experiment 1: Addition of anhydrous copper(II) sulfate
The temperature change is 8.4 oC
Experiment 2: Addition of hydrated copper(II) sulfate
The temperature change is 1.7oC
The enthalpy change for each reaction:
Experiment 1:
q = m x c x ΔT
q= 25 x 4.2 x 8.4 = 882 J = 0.882 kJ
n= 4.94 / 159.6 = 0.0310 mol
ΔH1 = q / n = 0.882 / 0.0310 = -28.45 kJ mol-1
Experiment 2:
q = m x c x ΔT
q= 25 x 4.2 x 1.7 = 178.5 J = -0.1785 kJ
n= 7.72 / 249.6 = 0.309
ΔH2 = q / n = 0.1785 / 0.309= +5.78 kJ mol-1
The enthalpy change, in kJ mol –1 for the hydration of copper(II) sulfate is:
ΔH3 = ΔH1 – ΔH2
ΔH3 = -28.45 -(+5.78 ) = -34.2 kJ mol-1
Examiner Tips and Tricks
Remember: The mass of the water would be 25 g as 25 cm3 of water is used and the density of water is 1 g cm-3.
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