Question

g Solid copper sulfide and silver nitrate react to form copper (II) nitrate and solid silver sulfide. Write a balanced chemical equation that describes the reaction. Identify the oxidation number of each element in the reaction as well as the physical state of each compound. You do not need to include the total contribution of charge. Is this reaction a redox reaction or a non-redox reaction

Answer 1

Answer:

$Cu^{2+}S^{2-}(s)+2Ag^+N^{5+}O^{2-}_3(aq)\rightarrow Cu^{2+}(N^{5+}O^{2-}_3)_2(aq)+Ag^+_2S^{2-}(s)$

It is a non-redox reaction.

Explanation:

Hello.

In this case, when solid copper sulfate and aqueous silver nitrate react to form solid silver sulfide and aqueous solid silver sulfide we can write:

$CuS(s)+2AgNO_3(aq)\rightarrow Cu(NO_3)_2(aq)+Ag_2S(s)$

In which the oxidation states are assigned based on the periodic table and taking into account that the left-handed ion is positively charged whereas the right-handed one is negatively charged:

$Cu^{2+}S^{2-}(s)+2Ag^+N^{5+}O^{2-}_3(aq)\rightarrow Cu^{2+}(N^{5+}O^{2-}_3)_2(aq)+Ag^+_2S^{2-}(s)$

Thus, since the oxidation states do not change from reactants to products, we infer this is a non-redox reaction.

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