Consider a galvanic cell based upon the following half reactions: 2+ Ni2 + 2eNi

Question

Consider a galvanic cell based upon the following half reactions: 2+ Ni2 + 2eNi 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 not change the potential of the cell 2. Decreasing the mass of the Cr will change the initial potential of the cell 3. Ni2+ is being reduced 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 2 5

Explanation / Answer

Cell reaction is,

3 Ni2+ (aq.) + 2 Cr (s) -----------> 2 Cr3+ (aq.) + 3 Ni (s)

Since, E0Ni2+/Ni > E0Cr3+/Cr, Ni2+ undergoes reduction .

Nernst equation,

Ecell = E0cell - (0.05916 / 6)*Log[Cr3+]2/[Ni2+]3

TRUE Options:

3. Ni2+ is being reduced during the reaction

4. Decrease in concentration of Ni2+ will decrease the potential of the cell

So, only 2 options are correct.

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