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romanna [79]
3 years ago
11

Be sure to answer all parts. Consider the following balanced redox reaction (do not include state of matter in your answers): 2C

rO2−(aq) + 2H2O(l) + 6ClO−(aq) → 2CrO42−(aq) + 3Cl2(g) + 4OH−(aq) (a) Which species is being oxidized? (b) Which species is being reduced?
Chemistry
1 answer:
timurjin [86]3 years ago
8 0

Answer:

The specie which is oxidized is:- CrO_2^-

The specie which is reduced is:- ClO^-

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^-

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