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

Options

A. `93000C `
B. `1.93 xx 10^(5) C`
C. `9.65 xx 10^(4) C`
D. `19.3 xx 10^(3) C`.

Answer

B

Explanation

`H_(2)O_(2) to H_(2)O + (1)/(2) O_(2)`
Oxidation of 1 mole of `H_(2)O_(2)` means both `O^(-)` ions should change to `O_(2)` ,
i.e,`2 O^(-) to O_(2) + 2e^(-)`
Thus , 1 mole of `H_(2)O_(2)` requires = 2 F = `2 xx 96500 C = 1.93 xx 10^(5)` C
(Remember that the given reaction is a disproportionation reaction `2H_(2)O_(2) to 2H_(2)O + O_(2)` in which 1 mole is reduced) ,
`H_(2)O_(2) to H_(2)O + (O)`
and 1 mole is oxidized ,
`H_(2)O_(2) + (O) to H_(2)O + O_(2)`