Question

How many coulombs of electrical charge is required for the oxidation of $1mole$ of $H_{2}O$ to $O_2$?

• A. $9.65\times {10}^{4}C$
• B. $4.825\times {10}^{5}C$
• C. $1.93\times {10}^{5}C$
• D. $1.93\times {10}^{4}C$

Answer 1

The correct option is C $1.93\times {10}^{5}C$

Given,

1 mole of $H_{2}O$ will produce one atom of $O$

$H_{2}O\to H_2+\frac{1}{2}{O}_2$

Charge on $O=-2$

$O_2^{-}\to \frac{1}{2}{O}_2+2e^{-}$

The electrical charge required for the oxidation of 1 mole of $H_{2}O$ to $O_2$

$Q=nF$

$Q=2\times 96487=1.92\times {10}^{5}C$

The correct option is C.