In alkaline medium, `ClO_(2)` oxidises `H_(2)O_(2) "to" O_(2)` and is itself reduced to `Cl^(ө)`. How many moles of `H_(2)O_(2)` are oxidised by `1 "mol of " ClO_(2)` ?

In alkaline medium ClO_(2) oxidises H_(2)O_(2) to O_(2) and it self gets reduces to Cl^-1 . How many moles of H_(2)O_(2) are oxidised by 1 mol of ClO_(2) ?

In alkaline medium CIO_(2) oxidises to H_(2)O_(2) and O_(2) and itself gets reduced to Cl^(-) . How many moles of H_(2)O_(2) are oxidised by 1 mole of ClO_(2) ? Hint: The balanced chemical equation is:

In alkaline medium , CIO_(2) oxidised by H_(2)O_(2) to O_(2) and itself reduces to CI^(-) ion .How many moles of H_(2)O_(2) will be oxidised by 1 mol of CIO_(2) ?