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Electrolysis and Electrolytes

Consider an e...

Question

Consider an electrochemical cell in which the following reaction occurs :
$F e^{2 +} (a q) + A g^{+} (a q) \to A g (s) + F e^{3 +} (a q)$
Then how many of following changes will decrease the cell voltage:

(i) Decrease the $[A g^{+}]$
(ii) Increase in $[F e^{3 +}]$
(III) Increase the amount of $A g$

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Solution

$F e^{2 +} (a q) + A g^{+} (a q) \to A g (s) + F e^{3 +} (a q) E_{c e l l} = E_{c e l l}^{o} - \frac{0.0591}{1} log \frac{[F e^{3 +}]}{[F e^{2 +}] [A g^{+}]}$
(i) By decreasing $[A g^{+}] \to E_{c e l l} ↓$
(ii) By increasing $[F e^{3 +}] \to E_{c e l l} ↓$
(iii) By increasing amount of $A g \to$ no effect on $E_{c e l l}$ .

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