The free energy change for the following reaction at 25 °C, when [Cd2+] = 1.20 M and [Fe2+] = 1.4010-3 M, is - 23.9 kJ: Cd2 + (1.20 M) + Fe (s) Cd (s) + Fe2 + (1.4010-3 M) ΔG = - 23.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: - 24.07 V Would this reaction be spontaneous in the forward or the reverse direction?

Question

Chemistry

Freddy Richard

4 May, 06:57

The free energy change for the following reaction at 25 °C, when [Cd2+] = 1.20 M and [Fe2+] = 1.4010-3 M, is - 23.9 kJ: Cd2 + (1.20 M) + Fe (s) Cd (s) + Fe2 + (1.4010-3 M) ΔG = - 23.9 kJ What is the cell potential for the reaction as written under these conditions? Answer: - 24.07 V Would this reaction be spontaneous in the forward or the reverse direction?

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Aspen · Answer 1

It's spontaneous in the reverse direction

Explanation:

A negative voltage indicate s that the reverse reaction is spontaneous (i. e. oxidation at the cathode, and reduction at the anode; by convention you would need to swap the labels on the electrodes)