Question

Balance the following reactions using either the oxidation number method or the half-reaction method. Identify which element has been oxidized and which has been reduced.
Ce4+ + I– → Ce3+ + IO3– (in a basic solution)

Answer 1

$6Ce^{4+} + I^- + 6OH^-$ → $6Ce^{3+} + IO_3^- + 3H_2O$ is the balanced chemical equation.

What is a balanced chemical equation?

A balanced chemical reaction is an equation that has equal numbers of each type of atom on both sides of the arrow.

Half-reaction method:

Unbalanced chemical equation:

$Ce^{4+} + I^-$→ $Ce^{3+} + IO^{3-}$

Oxidation half-reaction:

$I^-+ 6OH^- - 6e-$ → I$O^{3-} + 3H_2O$

Reduction half-reaction:

$Ce4^+ + e^-$ → $Ce^{3+}$

Balanced chemical equation:

$6Ce^{4+} + I^- + 6OH^-$→ $6Ce^{3+} + IO^{3-} + 3H_2O$

Oxidation number method:

Unbalanced chemical equation:

$Ce^{4+} + I^-$→ $Ce^{3+} + IO^{3-}$

$I^{-1} -6e^-$→ $I^{+5}$

$Ce^{4+} + e^-$ → $Ce^{3+}$

Balanced chemical equation:

$6Ce^{4+} + I^{-1}$ → $6Ce^{3+} + I^{+5}$

or

$6Ce^{4+} + I^- + 6OH^-$→ $6Ce^{3+} + IO_3^- + 3H_2O$

Hence, $6Ce^{4+} + I^- + 6OH^-$→ $6Ce^{3+} + IO_3^- + 3H_2O$ is the balanced chemical equation.

Learn more about the balanced chemical equation here:

https://brainly.in/question/46754758

#SPJ1