Question

For the reaction: $I^{-}+Cl{O}_3^{-}+H_{2}S{O}_4⟶C{l}^{-}+HS{O}_4^{-}+I_2$The correct statement(s) in the balanced equation is/are:

• A. Stoichiometric coefficient of $HS{O}_4^{-}$ is $6$
• B. Iodide is oxidized
• C. Sulphate is reduced
• D. $H_{2}O$ is one of the products.

Answer 1

The correct option is A Stoichiometric coefficient of $HS{O}_4^{-}$ is $6$

$I+Cl{O}_3+H_{2}S{O}_4⟶Cl+HS{O}_4+I_2$

$\to$ $I^{-}$ gets oxidised.

$\to$ $S{O}_4$ neither gets oxidised nor reduced.

$\to$ Clear from the equation $H_{2}O$ is not produced.

Balance equation:

$6I^{-}+Cl{O}_3^{-}+6H_{2}S{O}_4⟶C{l}^{-}+6HS{O}_4^{-}+3I_2+3H_{2}O$

$\therefore$ Stoichiometric coefficient of $HS{O}_4^{-}$ is $6$.