Answer:
Option A,B,D
Explanation:
Plan. This problem includes the concept of redox reaction. A redox reaction consists of oxidation half-cell reaction and reduction half-cell reaction.
Write both half-cell reactions, i.e, oxidation half-cell reaction and reduction half-cell reaction.
Then balance both the equations.
Now determine the correct value of stoichiometry of H2SO4.
Oxidation half-reaction.
$2I^{-}\rightarrow I_{2}+2e^{-}$ ..........(i)
Here, I- is converted into I2. The oxidation number of I is increasing from -1 to 0 hence, this is a type of oxidation reaction.
Reduction half-reaction.
$6H^{+}+ClO_3^-+6e^{-}\rightarrow Cl^{-}+3H_{2}O$ ............(ii)
Here, H2O releases as a product. Hence , option (d) is correct.
Mutiplying equation (i) by 3 and adding in equation (ii)
$6I^{-}+ClO_3^-+6H^{+}\rightarrow Cl^{-}+3I_{2}+3H_{2}O$
$6I^{-}+ClO_3^-+6H_{2}SO_{4}\rightarrow Cl^{-}+3I_{2}+3H_{2}O+6HSO_4^-$
Stoichiormetric coefficient of HSO4- is 6
Hence, option (a), (b) and (d) are correct.
