Question

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?

Answer 1

The specie which is oxidized is:-
`CrO_2^-`

The specie which is reduced is:-
`ClO^-`

Step-by-step explanation:

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.

`X\rightarrow X^(n+)+ne^-`

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.

`X^(n+)+ne^-\rightarrow X`

For the given chemical reaction:

`2CrO_2^- + 6ClO^- + 2H_2O\rightarrow 2CrO_4^(2-) + 3Cl_2 + 4OH^-`

The half cell reactions for the above reaction follows:

Oxidation half reaction:
`CrO_2^- + 2H_2O + 4OH^-\rightarrow CrO_4^(2-) + 4H_2O + 3e^-`

Reduction half reaction:
`2ClO^- + 4H_2O + 2e^-\rightarrow Cl_2 + 2H_2O + 4OH^-`

Thus, the specie which is oxidized is:-
`CrO_2^-`

The specie which is reduced is:-
`ClO^-`