H_(2)O_(2)" will oxidise "

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) ?

In a titration, H_(2)O_(2) is oxidised to O_(2) by MnO_(4)^(-) . 24 mL of 0.1M H_(2)O_(2) requires 16 mL of 0.1M MnO_(4)^(-) solution. Hence MnO_(4)^(-) changes to :

In a titration, H_(2)O_(2) is oxidised to O_(2) by MnO_(4)^(-) . 24 mL of 0.1M H_(2)O_(2) requires 16 mL of 0.1M MnO_(4)^(-) solution. Hence MnO_(4)^(-) changes to :

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, 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 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 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: