How many coulombs are required to oxidise 0.1 | vedclass

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(B) The oxidation reaction of water is: $H_2O \longrightarrow \frac{1}{2}O_2 + 2H^+ + 2e^-$. From the stoichiometry of the reaction,$1 \ mole$ of $H_2

Vedclass · Accepted Answer

$1.93 	imes 10^4 \ C$

Vedclass · Answer

(B) The oxidation reaction of water is: $H_2O \longrightarrow \frac{1}{2}O_2 + 2H^+ + 2e^-$. From the stoichiometry of the reaction,$1 \ mole$ of $H_2O$ requires $2 \ moles$ of electrons for oxidation. Since $1 \ mole$ of electrons carries $96500 \ C$ (Faraday's constant),$2 \ moles$ of electrons carry $2 	imes 96500 \ C = 193000 \ C$. Therefore,for $0.1 \ mole$ of $H_2O$,the charge required is $0.1 	imes 193000 \ C = 19300 \ C$. This is equal to $1.93 	imes 10^4 \ C$.

How many coulombs are required to oxidise $0.1 \ mole$ of $H_2O$ to oxygen?

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