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(C) The decomposition reaction is: $H_2O_{(l)} \rightarrow H_{2(g)} + \frac{1}{2} O_{2(g)}$.For the electrolysis of $H_2O$,the half-reaction at the an

Vedclass · Accepted Answer

$96500$

Vedclass · Answer

(C) The decomposition reaction is: $H_2O_{(l)} ightarrow H_{2(g)} + \frac{1}{2} O_{2(g)}$.For the electrolysis of $H_2O$,the half-reaction at the anode is $H_2O ightarrow \frac{1}{2} O_2 + 2H^+ + 2e^-$.Thus,$1 \ mol$ of $H_2O$ requires $2 \ mol$ of electrons for decomposition.For $2 \ mol$ of $H_2O$,the total charge required is $Q = n 	imes F = (2 	imes 2) 	imes 96500 \ C = 4 	imes 96500 \ C$.Using the formula $Q = I 	imes t$,where $I = 4 \ A$:$4 	imes 96500 = 4 	imes t$$t = 96500 \ s$.Therefore,the correct option is $C$.

How much time is required for the complete decomposition of $2 \ mol$ of $H_2O$ using a current of $4 \ A$?

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