Consider the following balanced redox reaction (do not include state of matter in your answers): 2cro2-(aq) + 2h2o(l) + 6clo-(aq) rightarrow 2cro42- (aq) + 3cl2(g) + 4oh-(aq) which species is being oxidized? which species is being reduced? which species is the oxidizing agent?

CrO₂⁻

ClO⁻

ClO⁻

Explanation:

Let's consider the following redox reaction.

2 CrO₂⁻(aq) + 2 H₂O(l) + 6 ClO⁻(aq) → 2 CrO₄²⁻(aq) + 3 Cl₂(g) + 4 OH⁻(aq)

We can identify both half-reactions.

Reduction: 6 H₂O(l) + 6 ClO⁻(aq) + 6 e⁻ → 3 Cl₂(g) + 12 OH⁻(aq)

Oxidation: 8 OH⁻(aq) + 2 CrO₂⁻(aq) → 2 CrO₄²⁻(aq) + 4 H₂O(l) + 6 e⁻

Which species is being oxidized?

CrO₂⁻ is being oxidized. Its oxidation number increases from +3 to +6.

Which species is being reduced?

ClO⁻ is being reduced. Its oxidation number decreases from +1 to 0.

Which species is the oxidizing agent?

The species being reduced is the oxidizing agent, that is, ClO⁻.

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.

ok whats the question if not i cannot you i need question and need a thing to answer