step by step balancing of redox reaction
KClO3+H2SO4 -->KHSO4+HClO4+ClO2+H2O
ionic equation :-
ClO3^-1 ----------> Clo4^-1 + ClO2
oxidation reaction :-
oxidation number of Cl in Clo3^-1 is +5 and oxidation number of Clorine in Clo4^-1 is +7
here oxidation number of clorine is increasing so its a oxidation reaction
ClO3^-1 -----> ClO4^-1
Balance the oxidation reaction by adding the electron
ClO3^-1 -----> ClO4^-1 + 2e^-1 -------------(1)
(oxidation number of clorine is changing + 5 to + 7 so add 2 electron there to balance the reaction )
reduction reaction :-
oxidation number of Clrine in ClO3^-1 is +5 and in ClO2 oxidation number is +4, oxidation number is decreasing hence this is
a reduction reaction
ClO3^-1 ------> ClO2
ClO3^-1 + e^-1 -------> ClO2 -------------(2)
(oxidation number of clorine is changing + 5 to + 4 so add 1 electron there to balance the reaction )
multiply by 2 in second equation to make same number of electron in both equation first and second
2ClO3^-1 + 2e^-1 -------> 2ClO2 -------------(3)
add equation first and third we get
ClO3^-1 + 2ClO3^-1 + 2e^-1 ----------> Clo4^-1 + 2ClO2 + 2e^-1
calcel out the electron we get
ClO3^-1 + 2ClO3^-1 ----------> Clo4^-1 + 2ClO2
H2SO4 is an acid and in acidic redox reaction we always balance the reaction using H+ ions
So balance the charge using H+ ions
ClO3^-1 + 2ClO3^-1 + 2H+ ----------> Clo4^-1 + 2ClO2
now Add H2O to balance the complete reaction
ClO3^-1 + 2ClO3^-1 + 2H+ ----------> Clo4^-1 + 2ClO2 + H2O
Answer :-
3ClO3^-1 + 2H+ ----------> Clo4^-1 + 2ClO2 + H2O