Be sure to answer all parts. Consider the following balanced redox reaction (do not include state of matter in your answers): 2CrO2−(aq) + 2H2O(l) + 6ClO−(aq) → 2CrO42−(aq) + 3Cl2(g) + 4OH−(aq) (a) Which species is being oxidized? (b) Which species is being reduced?

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

[tex]X\rightarrow X^{n+}+ne^-[/tex]

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

[tex]X^{n+}+ne^-\rightarrow X[/tex]

For the given chemical reaction:

[tex]2CrO_2^- + 6ClO^- + 2H_2O\rightarrow 2CrO_4^{2-} + 3Cl_2 + 4OH^-[/tex]

The half cell reactions for the above reaction follows:

Oxidation half reaction: [tex]CrO_2^- + 2H_2O + 4OH^-\rightarrow CrO_4^{2-} + 4H_2O + 3e^-[/tex]

Reduction half reaction: [tex]2ClO^- + 4H_2O + 2e^-\rightarrow Cl_2 + 2H_2O + 4OH^-[/tex]

Thus, the specie which is oxidized is:- [tex]CrO_2^-[/tex]

The specie which is reduced is:- [tex]ClO^-[/tex]