Question

Consider a galvanic cell based upon the following half reactions: Ni2+ + 2e- → Ni -0.27...

Consider a galvanic cell based upon the following half reactions:

Ni2+ + 2e- → Ni -0.27 V

Cr3+ + 3e- → Cr -0.73 V

How many of the following responses are true?

1. Adding equal amounts of water to both half reaction vessels will decrease the potential of the cell

2. Increasing the mass of the Ni will change the initial potential of the cell

3. Cr is being oxidized during the reaction

4. Decreasing the concentration of Ni2+ (assuming no volume change) will decrease the potential of the cell

5. Decreasing the concentration of Cr3+ (assuming no volume change) will decrease the potential of the cell

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Answer #1

3. Cr acts as anode. So, it will be oxidized. So, it is TRUE.

4. As Concentration of Ni2+ is in denominator. So, decreasing its concentration will decrease the concentration factor of Nernst equation. So, cell potential will decrease. Hence, this statement is TRUE.

5.Decrease in concentration of Cr3+ will increase the cell potential. Hence, this statement is FALSE.

So, correct statements are 1), 3) and 4).

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