# Problem: Given the following two half reactions and their potentials, which net reaction is spontaneous? Zn2+(aq) + 2 e– → Zn(s)      E°cell = –0.763 VNi2+(aq) + 2 e– → Ni(s)        E°cell = –0.25 VA. Zn2+(aq) + Ni(s) → Zn(s) + Ni2+(aq)B. Ni2+(aq) + Zn(s) → Ni(s) + Zn2+(aq)C. Ni(s) + Zn(s) → Zn2+(aq) + Ni2+(aq)D. Zn2+(aq) + Ni2+(aq) → Ni(s) + Zn(s) E. Zn2+(aq) + Zn(s) → Ni(s) + Ni2+(aq)

###### FREE Expert Solution

We’re being asked to determine the net reaction that is spontaneous.

We're given the following

Zn2+(aq) + 2 e → Zn(s)      E°cell = –0.763 V
Ni2+(aq) + 2 e → Ni(s)        E°cell = –0.25 V

Recall that the greater the E°cell of a redox reaction, the more likely the reaction will occur (more spontaneous reaction)

E°cell > 0 spontaneous in the forward direction
E°cell < 0 nonspontaneous in the forward direction

Determine the anode and cathode by comparing their E° values.

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###### Problem Details

Given the following two half reactions and their potentials, which net reaction is spontaneous?

Zn2+(aq) + 2 e → Zn(s)      E°cell = –0.763 V
Ni2+(aq) + 2 e → Ni(s)        E°cell = –0.25 V

A. Zn2+(aq) + Ni(s) → Zn(s) + Ni2+(aq)

B. Ni2+(aq) + Zn(s) → Ni(s) + Zn2+(aq)

C. Ni(s) + Zn(s) → Zn2+(aq) + Ni2+(aq)

D. Zn2+(aq) + Ni2+(aq) → Ni(s) + Zn(s)

E. Zn2+(aq) + Zn(s) → Ni(s) + Ni2+(aq)