Question

SO42- + 2Cr(OH)3 + 4OH- → + 2CrO42- + 3SO32- + 5H2O

In the above redox reaction. Use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.

Answer 1

Reduced species and oxidizing agent: sulfur in the form of sulfate.

Oxidized species and reducing agent: chromium in the form of chromous hydroxide.

Step-by-step explanation:

Hello!

In this case, for the reaction:

`SO_4^(2-) + 2Cr(OH)_3 + 4OH^- \rightarrow 2CrO_4^(2-) + 3SO_3^(2-) + 5H_2O`

We can see that the oxidation states of sulfur and chromium change from +6 to +4 and +3 to +6 respectively; in such a way, since the oxidized species is the same reducing agent because it undergoes an increase in the oxidation state, we infer that chromium is it as it goes from +3 to +6.

Moreover, since the reduced species is the same oxidizing agent because it undergoes a decrease in the oxidation state, we infer that sulfur is it as it goes from +6 to +4.

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