Ncert Exercises & Solutions

Mg_(s) | Mg²⁺_(0.001M) || Cu²⁺_{(0.0001 M)} | Cu_(s)

$E_{{Mg}^{2 +} / Mg}^{o} = - 2.36 V; E_{{Cu}^{2 +} / Cu}^{o} = 0.34 V$ $E_{{Mg}^{2 +} / Mg}^{o} = - 2.36 V; E_{{Cu}^{2 +} / Cu}^{o} = 0.34 V$

The value of $E_{cell}$ $E_{cell}$ for the above reaction is -

1.	3.46 V	2.	3.15 V
3.	2.67 V	4.	1.24 V

Hint:

$E_{cell} = E_{cell}^{⊝} - \frac{0.0591}{n} \log \frac{[{Mg}^{2 +}]}{[{Cu}^{2 +}]}$

Step 1:

Calculate the value of

$E_{cell}^{o}$ as follows:

$E_{cell}^{⊝} = E_{Mg / {Mg}^{2 +}}^{o} + E_{{Cu}^{2 +} / Cu}^{o}$

$E_{cell}^{⊝} = 2.36 + 0.34 V$

$E_{cell}^{⊝} = 2.70 V$

Step 2:

Calculate the value of

$E_{cell}$ as follows:

$E_{cell} = E_{cell}^{⊝} - \frac{0.0591}{n} \log \frac{[{Mg}^{2 +}]}{[{Cu}^{2 +}]}$

$= {0.34 - (- 2.36)} - \frac{0.0591}{2} \log \frac{. 001}{. 0001}$

$= 2.7 - \frac{0.0591}{2} \log 10$

=2.7 - 0.02955

=2.67 V (approximately)