Electrochemistry Result Question 26
Passage
The electrochemical cell shown below is a concentration cell. $M \mid M^{2+}$ (saturated solution of a sparingly soluble salt, $\left.M X_2\right)|| M^{2+}\left(0.001 \mathrm{mol} \quad \mathrm{dm}^{-3}\right) \mid M$. The emf of the cell depends on the difference in concetration of $M^{2+}$ ions at the two electrodes. The emf of the cell at $298 K$ is $0.059 V$ .
(2012)
26. The value of $\Delta G\left(\mathrm{~kJ} \mathrm{~mol}^{-1}\right)$ for the given cell is (take $1 \mathrm{~F}=96500 \mathrm{C} \mathrm{mol}^{-1}$ )
(a) -5.7
(b) 5.7
(c) 11.4
(d) -11.4
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Answer:
Correct Answer: 26. ( d )
Solution:
- $\Delta G=-n E F=-\frac{2 \times 0.059 \times 96500}{1000} \mathrm{kJ}=-11.4 \mathrm{kJ}$
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