When a current of 2 A is passed through a mo | vedclass

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(C) According to Faraday's law of electrolysis,the mass deposited $w = \frac{I 	imes t 	imes M}{n 	imes F}$.Given: $w = 22.2 \ g$,$I = 2 \ A$,$t =

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$+2$

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(C) According to Faraday's law of electrolysis,the mass deposited $w = \frac{I 	imes t 	imes M}{n 	imes F}$.Given: $w = 22.2 \ g$,$I = 2 \ A$,$t = 5 \ hours = 5 	imes 3600 \ s = 18000 \ s$,$M = 118.69 \ g/mol$,$F = 96500 \ C/mol$.Substituting the values: $22.2 = \frac{2 	imes 18000 	imes 118.69}{n 	imes 96500}$.$n = \frac{2 	imes 18000 	imes 118.69}{22.2 	imes 96500} \approx \frac{4272840}{2142300} \approx 1.994 \approx 2$.Therefore,the oxidation state of tin is $+2$.

When a current of $2 \ A$ is passed through a molten tin salt for $5 \ hours$,$22.2 \ g$ of tin is deposited. What is the oxidation state of tin in the salt? (Atomic weight of $Sn = 118.69$)

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