1 Faraday electricity was passed through Cu²⁺ (1.5 M, 1 L)/Cu and 0.1 Faraday was passed through Ag⁺ (0.2 M, 1…

Question

1 Faraday electricity was passed through $\text{Cu}^{2+}$ ( $1.5 \, \text{M}$ , $1 \, \text{L}$ )/Cu and $0.1$ Faraday was passed through $\text{Ag}^+$ ( $0.2 \, \text{M}$ , $1 \, \text{L}$ ) electrolytic cells. After this, the two cells were connected as shown below to make an electrochemical cell. The emf of the cell thus formed at $298 \, \text{K}$ is _____ mV. (Nearest integer)

Electrochemical cell diagram with copper electrode in Cu2+ aqueous solution on left, silver electrode in Ag+ aqueous solution on right, connected by a salt bridge and external circuit with galvanometer.

Given: $E^\circ_{\text{Cu}^{2+}/\text{Cu}} = 0.34 \, \text{V}$ $E^\circ_{\text{Ag}^+/ \text{Ag}} = 0.8 \, \text{V}$ $\frac{2.303RT}{F} = 0.06 \, \text{V}$

Given: $$E^\circ_{	ext{Cu}^{2+}/	ext{Cu}} = 0.34 \, 	ext{V}$$ $$E^\circ_{	ext{Ag}^+/ 	ext{Ag}} = 0.8 \, 	ext{V}$$ $$\frac{2.303RT}{F} = 0.06 \, 	ext{V}$$

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400

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