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(B) The decomposition reaction of water is $H_2O \rightarrow H_2 + \frac{1}{2}O_2$. In this reaction,the oxidation of $O^{2-}$ to $O_2$ involves $2 \,

Vedclass · Accepted Answer

$1.93 	imes 10^5 \, 	ext{sec}$

Vedclass · Answer

(B) The decomposition reaction of water is $H_2O ightarrow H_2 + \frac{1}{2}O_2$. In this reaction,the oxidation of $O^{2-}$ to $O_2$ involves $2 \, e^-$ per mole of $H_2O$ $(O^{2-} ightarrow \frac{1}{2}O_2 + 2e^-)$. For $4 \, 	ext{moles}$ of water,the total charge $Q$ required is $Q = n 	imes 	ext{moles} 	imes F = 2 	imes 4 	imes 96500 \, 	ext{C} = 772000 \, 	ext{C}$. Using the formula $Q = I 	imes t$,where $I = 4 \, 	ext{A}$,we get $772000 = 4 	imes t$. Therefore,$t = \frac{772000}{4} = 193000 \, 	ext{sec} = 1.93 	imes 10^5 \, 	ext{sec}$.

How much time is required for complete decomposition of $4 \, \text{moles}$ of water using $4 \, \text{A}$ current?

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