Question

Which of the following reactions would be classified as oxidation-reduction? Check all that apply. View Available Hint(s) Check all that apply. 2Na(s)+Cl2(g)→2NaCl(s) Na(s)+CuCl(aq)→NaCl(aq)+Cu(s) NaCN(aq)+CuCl(aq)→NaCl(aq)+CuCN(s)

Answer 1

Answer:The 1st and 2nd reactions are the example of oxidation -reduction.

Explanation:

Oxidation is basically when a species  loses electrons and  reduction is basically when the species gains  electrons.

A reaction is known as an oxidation -reduction reaction only if  oxidation and reduction simultaneously occur in the reaction. It basically means if a species is getting oxidized in the reaction then the other species present in the system must be reduced in the reaction.

Oxidation-reduction reactions are also known as redox reactions.

In the 1st reaction the oxidation state of Na in reactant is 0 and in products is +1 hence Na is oxidized and the oxidation state of   chlorine is  0 in reactants and  in products is  -1 so chlorine is reduced. Hence Na is oxidized and Cl is reduced so the reaction is a example of oxidation-reduction.

2Na(s)+Cl₂(g)→2NaCl(s)

In the second reaction the oxidation state of Na in reactant is 0 and in products is +1 hence Na is oxidized and the oxidation state of Cu is +1 in reactant and 0 in products so Cu is reduced. Hence Na is oxidized and Cu is reduced so the reaction is an example of oxidation-reduction.

Na(s)+CuCl(aq)→NaCl(aq)+Cu(s)

In the third reaction the oxidation state of Na changes from +1 to +1 and that of Cu also changes from +1 to +1. So there is no change in oxidation state of the species present in reactants and products. Hence this reaction is not an example of oxidation and reduction.