Question

E. 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. (you do not need to include the total contribution of charge.) is this reaction a redox reaction or a non-redox reaction? explain your answer.

Answer 1

It is reaction of ion exchange. Substances react in the melt. As a result we receive alloy of four salts.

CuS + 2AgNO₃ ⇄ Cu(NO₃)₂ + Ag₂S

Answer 2

Answer:

The given reaction is not a redox reaction.

Explanation:

Redox reaction is defined as chemical reaction in oxidation and reduction reactions occurs simultaneously.

Oxidation reaction is defined as the reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.

Reduction reaction is defined as the reaction in which an atom gains electrons. Here, oxidation state of the atom decreases.

Solid copper sulfide when immersed in silver nitrate solution it reacts to form silver sulfide precipitate and copper(II) nitrate solution.

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

Oxidation states of elements on reactant side:

Oxidation state of copper  = +2

Oxidation state of sulfur = -2

Oxidation number of silver  +1

Oxidation number of nitrogen = +5

Oxidation number of oxygen = -2

Oxidation states of elements on product side:

Oxidation state of copper  = +2

Oxidation state of sulfur = -2

Oxidation number of silver  +1

Oxidation number of nitrogen = +5

Oxidation number of oxygen = -2

No change in oxidation states of elements is observed which means that the given reaction is not a redox reaction.