Part 1 Which of the following is a redox reaction?

a. H2CO3 (aq) + 2NH3 (aq) → 2NH4+ (aq) + CO32- (aq)



b. 2VO3- (aq) + Zn (s) + 8H+ (aq) → 2VO2+ (aq) + Zn2+ (aq) + 4H2O (l)



d. Zn(NO) (aq) + 2NaOH (aq) → Zn(OH) (s) + 2NaNO (aq)

part 2 For the redox reaction in part 1 , which substance is oxidized? Which is reduced?

More specific labeling of the subject would be more likely to attract tutors with expertise in this area.

To determine which of the given reactions is a redox reaction, we need to identify if there is a change in oxidation states for any of the elements involved.

a. H2CO3 (aq) + 2NH3 (aq) → 2NH4+ (aq) + CO32- (aq)
In this reaction, there is no change in oxidation states for any of the elements. The oxidation state of each element remains the same throughout, so this is not a redox reaction.

b. 2VO3- (aq) + Zn (s) + 8H+ (aq) → 2VO2+ (aq) + Zn2+ (aq) + 4H2O (l)
In this reaction, the oxidation state of vanadium (V) changes from +5 in VO3- to +4 in VO2+. The oxidation state of zinc (Zn) changes from 0 in the solid state to +2 in Zn2+. Therefore, this reaction is a redox reaction.

d. Zn(NO) (aq) + 2NaOH (aq) → Zn(OH) (s) + 2NaNO (aq)
It appears that this reaction is incomplete or contains errors. The chemical formula Zn(NO) and Zn(OH) are not conventionally used, so it is difficult to determine the oxidation states of zinc. Therefore, it is not possible to classify this reaction as a redox reaction without accurate chemical formulas.

For the redox reaction in part 1 (b), vanadium (V) is oxidized because its oxidation state decreases from +5 to +4. Zinc is reduced because its oxidation state increases from 0 to +2.