Answer:
Reduced species and oxidizing agent: sulfur in the form of sulfate.
Oxidized species and reducing agent: chromium in the form of chromous hydroxide.
Explanation:
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In this case, for the reaction:
[tex]SO_4^{2-} + 2Cr(OH)_3 + 4OH^- \rightarrow 2CrO_4^{2-} + 3SO_3^{2-} + 5H_2O[/tex]
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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