Question 21.9: Write a balanced net ionic equation for the reaction of nitr...
Write a balanced net ionic equation for the reaction of nitric acid with insoluble copper(II) sulfide; the products include Cu^{2+}, S(s), and NO_{2}(g).
STRATEGY
1. Recall the general procedure for writing and balancing redox equations from Chapter 4.
2. Note that HNO_{3} is a strong acid, so it should be represented as H^{+} and NO_{3}^{-} ions.
| oxidation: CuS(s) → S(s) reduction: NO_{3}^{-}(aq) → NO_{2}(g) |
Skeleton half-equations |
| oxidation: CuS(s) → S(s) + Cu^{2+}(aq) + 2 e^{-} reduction: NO_{3}^{-}(aq) + 2H^{+}(aq) + e^{-}(aq) → NO_{2}(g) + H_{2}O |
Balanced half-reactions |
| CuS(s) → S(s) + Cu^{2+}(aq) + 2e^{-}
\frac{2(NO_{3}^{-}(aq) + 2H^{+}(aq) + e^{-}(aq) → NO_{2}(g) + H_{2}O)}{CuS(s) + 2NO_{3}^{-}(aq) + 4H^{+}(aq) → Cu^{2+}(aq) + S(s) + 2NO_{2}(g) + 2H_{2}O} |
Overall reaction |
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