How many coulombs are required for the oxidation of `1 mol` of `H_(2)O` to `O_(2)`?

Options

A. `9.65 xx10^(4)`C
B. `1.93 xx 10^(4)`C
C. `1.93 xx10^(5)` C
D. `19.3 xx10^(5)` C

Answer

C

Explanation

The electrode reaction for 1 mole of `H_(2)O` is
`H_(2)O rarr H_(2)+1/2 O_(2), O^(2-) rarr1/2 O_(2) +2e^(-)`
`2H^(+)+2e^(-)rarr H_(2)` or `H_(2)O rarr 2E^(+)+1/2 O_(2) +2e^(-)`
Electricity required for oxidation of 1 mole of `H_(2)O= 2F`
1 F =96500C
`therefore` Total charge `=2xx96500=1.93 xx10^(5) c`