First slide

Nernst Equation

Question

The standard reduction potentials of Zn²⁺ | Zn and Cu²⁺ | Cu are –0.76 V and + 0.34 V respectively. What is the cell e.m.f (in V) of the following cell?
Zn | Zn²⁺ (0.05 M || Cu²⁺ (0.005 M | Cu.

Moderate

A

1.1295
B

1.0705
C

1.1
D

1.041

Solution

$Zn + {Cu}^{2 +} (0.005 M) \to {Zn}^{2 +} (0.05 M) + Cu;$
Applying Nernst equation
$E_{cell} = (E_{c}^{o} - E_{a}^{o}) - \frac{0.0591}{2} \log \frac{[{Zn}^{+ 2}]}{[{Cu}^{+ 2}]}$
$E_{cell} = (0.34 + 0.76) - \frac{0.0591}{2} \log \frac{[0.05]}{[0.005]} = 1.1 - 0.03 = 1.07 V$

Get Instant Solutions

When in doubt download our app. Now available Google Play Store- Doubts App

Recieve an sms with download link

Doubts App

OR

SCAN ME

Doubts App

Doubts App