Question

5) Which species is oxidized in the reaction below?

Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l)

H+, N+5, O2-, H2O, Au

A) H+

B) N+5

C) Au

D) O2-

E) H2O

Answer 1

Answer on Question #73737 – Chemistry – Other

Task:

5) Which species is oxidized in the reaction below?

$$\mathrm{Au}(\mathrm{s}) + 3\mathrm{NO}_3^-(\mathrm{aq}) + 6\mathrm{H}^+(\mathrm{aq}) \rightarrow \mathrm{Au}^{3+}(\mathrm{aq}) + \mathrm{NO}(\mathrm{g}) + 3\mathrm{H}_2\mathrm{O} (\mathrm{l})$$

A) $\mathrm{H}^+$;

B) $\mathrm{N}^{+5}$;

C) Au;

D) $\mathrm{O}^{2-}$;

E) $\mathrm{H}_2\mathrm{O}$;

Solution:

$$\mathrm{Au}(\mathrm{s}) + 3\mathrm{NO}_3^-(\mathrm{aq}) + 6\mathrm{H}^+(\mathrm{aq}) = \mathrm{Au}^{3+}(\mathrm{aq}) + \mathrm{NO}(\mathrm{g}) + 3\mathrm{H}_2\mathrm{O}$$ $$\mathrm{Au}^0 - 3\mathrm{e} = \mathrm{Au}^{3+} \quad - \text{oxidized}$$ $$\mathrm{N}^{+5} + \mathrm{e} = \mathrm{N}^{+4} \quad - \text{reduced}$$

Au – Reducing agent. Reducing agents are oxidized

Answer: C) Au.

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