Consider the following galvanic cell: Pt|Cr^3 (0.30 M), Cr^2+ (0.030 M) || AgCl(

Question

Consider the following galvanic cell: Pt|Cr^3 (0.30 M), Cr^2+ (0.030 M) || AgCl(s), Cl (0.025 M) |Ag For each of the following experiments, will the voltage of the cell increase, decrease, or be unchanged? Addition of 10 grams of solid silver chloride to the right half-cell. Dissolution of 10 grams of sodium chloride in the right half-cell. Addition of 10 mL of water to the left half-cell. Addition of some soluble chromium(II) salt to the left half-cell. Dissolution of some silver nitrate in the right half-cell.

Explanation / Answer

(a). Adding 10 grams of solid silver chloride to the right half cell, will not affect the concentration in the right half cell.

So the voltage of the cell will be unchanged.

(b). Dissolution of 10 grams of sodium chloride in the right half cell will increase the Cl- concentration. The value of Q will become greater than 1.0 and the log term in the Nernst equation will become positive.

So the voltage of the cell will decrease.

(c). Addition of 10 mL of water to the left half cell will decrease the concentration on the left side. The value of Q will become greater than 1.0 and the log term in the Nernst equation will become positive.

So the voltage of the cell will decrease.

(d). Addition of some soluble chromium (II) salt to the left half cell will increase the concentration on the left side. The value of Q will become less than 1.0 and the log term in the Nernst equation will become negative.

So the voltage of the cell will increase.

(e). Dissolution of some silver nitrate in the right half cell will will decrease the Cl- concentration. The value of Q will become less than 1.0 and the log term in the Nernst equation will become negative.

So the voltage of the cell will increase.

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