Problem: The nickel­cadmium battery cell has a standard potential of +1.20 V. The cell reaction is2 NiO(OH)(s) + Cd(s) + 2 H2O(l) → 2 Ni(OH)2(s) + Cd(OH)2(s).What is the standard free energy change (kJ) for this reaction?a. -347 kJb. +116 kJc. -116 kJd. +232 kJe. -232 kJ

FREE Expert Solution

We’re being asked to calculate for the standard free energy change, ΔG° (kJ) for this reaction:

2 NiO(OH)(s) + Cd(s) + 2 H2O(l) → 2 Ni(OH)2(s) + Cd(OH)2(s)     E°cell = +1.20 V


ΔG° can be calculated from the cell potential using the following equation:

G=-nFE°cell

ΔG° = Gibbs Free Energy, J
n = # of e- transferred
F = Faraday’s constant = 96485 J/(mol e-)
cell = standard cell potential, V


First, let’s determine how many electrons were transferred from the cell reaction:

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Problem Details

The nickel­cadmium battery cell has a standard potential of +1.20 V. The cell reaction is

2 NiO(OH)(s) + Cd(s) + 2 H2O(l) → 2 Ni(OH)2(s) + Cd(OH)2(s).

What is the standard free energy change (kJ) for this reaction?

a. -347 kJ
b. +116 kJ
c. -116 kJ
d. +232 kJ
e. -232 kJ

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.