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)

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.

it should be p1 v1 = p2 v2

because of all the things that happen around the us, many people get into arguments which sadly could get physical, but we should actually make a change for that.