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:
ΔG° = Gibbs Free Energy, J
n = # of e- transferred
F = Faraday’s constant = 96485 J/(mol e-)
E°cell = standard cell potential, V
First, let’s determine how many electrons were transferred from the cell reaction:
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?
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Based on our data, we think this problem is relevant for Professor Marin's class at UCF.