First slide

Nernst Equation

Question

$\large {E^0}_{C{u^{2 + }}/Cu}\, = \, + 0.337\,V,$ , $\large {E^0}_{Z{n^{2 + }}/Zn}\, = \, - 0.762\,V,$ The EMF of the cell,
Zn | Zn²⁺ (0.1M) || Cu²⁺ (0.01M) | Cu is

Moderate

A

+1.099 V
B

– 1.099 V
C

+1.069 V
D

– 1.069 V

Solution

Metal electrode with High SRP is cathode and with low SRP is anode
Cell reaction
$Z{n_{\left( s \right)}} + Cu_{\left( {aq} \right)}^{ + 2} \rightleftharpoons Zn_{\left( {aq} \right)}^{ + 2} + C{u_{\left( s \right)}}$
Applying Nernst equation
${E_{cell}} = \left( {E_c^o - E_a^o} \right) - \frac{{0.0591}}{2}\log \frac{{\left[ {Z{n^{ + 2}}} \right]}}{{\left[ {C{u^{ + 2}}} \right]}}$
$= \left( {0.337 - \left( {0.762} \right)} \right) - \frac{{0.0591}}{2}\log \frac{{0.1}}{{0.01}} = 1.099 - 0.03 = 1.069V$

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