Electrochemistry 2 Question 27
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26. The value of $\Delta G\left(\mathrm{~kJ} \mathrm{~mol}^{-1}\right)$ for the given cell is ( take $1 \mathrm{~F}=96500 \mathrm{C} \mathrm{mol}^{-1}$ )
======= ####26. The value of $\Delta G\left(\mathrm{~kJ} \mathrm{~mol}^{-1}\right)$ for the given cell is ( take $1 \mathrm{~F}=96500 \mathrm{C} \mathrm{mol}^{-1}$ )
3e0f7ab6f6a50373c3f2dbda6ca2533482a77bed (a) -5.7
(b) 5.7
(c) 11.4
(d) -11.4
Passage II
The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal $M$ is :
$$ M(s) \mid M^{+}(\text {aq; } 0.05 \text { molar }) | M^{+}(a q ; 1 \text { molar }) \mid M(s) $$
For the above electrolytic cell the magnitude of the cell potential $\left|E_{\text {cell }}\right|=70 \mathrm{mV}$.
(2010)
Show Answer
Solution:
- $\Delta G=-n E F=-\frac{2 \times 0.059 \times 96500}{1000} \mathrm{~kJ}=-11.4 \mathrm{~kJ}$
