In alkanline medium `ClO_(2)` oxidises `H_(2)O_(2)` to `O_(2)` and itself gets reduced to `Cl^(-)`. How many moles of `H_(2)O_(2)` are oxidised by 1 mol of `ClO_(2)`?

Options

A. `1.0`
B. `1.5`
C. `2.5`
D. `3.5`

Answer

C

Explanation

`(({:(2ClO_(2)+2OH^(-)to2Cl^(-)+H_(2)O+5[O]),(H_(2)O_(2)+[O]toH_(2)O+O_(2)xx5):})/(5H_(2)O_(2)+2ClO_(2)+2OH^(-)to6H_(2)O+2Cl^(-)+5O_(2)))/`
Thus, one mole of `ClO_(2)` oxidises 5/2 or 2.5 moles of `H_(2)O_(2)`