In the balanced chemical reaction IO_3^- + aI | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The given unbalanced equation is: $IO_3^- + aI^- + bH^+ \longrightarrow cH_2O + dI_2$To balance the redox reaction:$1$. Oxidation half-reaction: $

Vedclass · Accepted Answer

$5, 6, 3, 3$

Vedclass · Answer

(A) The given unbalanced equation is: $IO_3^- + aI^- + bH^+ \longrightarrow cH_2O + dI_2$To balance the redox reaction:$1$. Oxidation half-reaction: $2I^- \longrightarrow I_2 + 2e^-$$2$. Reduction half-reaction: $IO_3^- + 6H^+ + 5e^- \longrightarrow \frac{1}{2}I_2 + 3H_2O$Multiplying the oxidation half-reaction by $5$ and the reduction half-reaction by $2$ to balance electrons:$10I^- \longrightarrow 5I_2 + 10e^-$$2IO_3^- + 12H^+ + 10e^- \longrightarrow I_2 + 6H_2O$Adding them together:$2IO_3^- + 10I^- + 12H^+ \longrightarrow 6I_2 + 6H_2O$Dividing by $2$ to simplify:$IO_3^- + 5I^- + 6H^+ \longrightarrow 3H_2O + 3I_2$Comparing with the given equation,we get $a=5, b=6, c=3, d=3$.Thus,the correct option is $A$.

In the balanced chemical reaction $IO_3^- + aI^- + bH^+ \longrightarrow cH_2O + dI_2$,the values of $a, b, c,$ and $d$ are respectively:

Similar Questions

Consider the following reaction:
$xMnO_4^{-} + yC_2O_4^{2-} + zH^{+} \rightarrow xMn^{2+} + 2yCO_2 + \frac{z}{2}H_2O$
The values of $x, y$ and $z$ in the reaction are,respectively:

The product of $I^-$ with $MnO_4^-$ in acidic medium is

When $SO_2$ gas is passed through an acidic solution of $K_2Cr_2O_7$,what is the change in the oxidation state of chromium?

What is the equivalent weight of $SnCl_{2}$ in the following reaction: $SnCl_{2} + Cl_{2} \longrightarrow SnCl_{4}$?

For the redox reaction $MnO_4^- + C_2O_4^{2-} + H^{+} \to Mn^{2+} + CO_2 + H_2O$,the correct coefficients of the reactants for the balanced reaction are:
$MnO_4^-$ : $C_2O_4^{2-}$ : $H^{+}$

Vedclass Test Series

Exam Paper Generator

Online Exam Module