Question

How many coulombs of electricity are required for the oxidation of 1 mole of $H_{2}O$ to $O_2$?

• A. $9.65\times {10}^{4}C$
• B. $4.825\times {10}^{4}C$
• C. $1.93\times {10}^{5}C$
• D. $3.86\times {10}^{5}C$

Answer 1

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

Oxidation of $H_{2}O$ to $O_2$ is:
$2H_{2}O\to 4H^{+}+O_2+4e^{-}$
Oxidation of 2 moles of water requires $96500\times 4C$
$\therefore$ oxidation of 1 mole of water requires $=\frac{96500\times 4}{2}=1.93\times {10}^{5}C$