Question

The amount of electricity in Coulomb required for the oxidation of 1 mol of \(H_2O\) to \(O_2\) is ____ \(\times 10 ^5 C.\)

Answer 1

Correct answer is : 2

\(2H_2 O \rightarrow O_2 +4 H^+ +4e^-\)

\(\frac {W}{E}=\frac {Q}{96500}\)

mole \(\times\) n-factor \(= \frac{Q}{96500}\)

\(1\times 2 = \frac {Q}{96500}\)

\(Q\times 2 \times 96500\,C\)

\(=1.93 \times 10 ^5 C\)