Label the following reactions as oxidation or reduction. Cr+3(aq) + 3e-s → Cr Ag(s) → 1e-s + Ag+1(ag) Mn(s) → 5e-s + Mn+5(aq) Sn+2(aq) + 2e-s → Sn

See the explanation

Explanation:

Our reactions for this question are:

a) Cr+3(aq) + 3e- → Cr(s)

b) Ag(s) → 1e- + Ag+1(ag)

c) Mn(s) → 5e- + Mn+5(aq)

d) Sn+2(aq) + 2e- → Sn(s)

Now, we have to remember the definition of oxidation and reduction. In a reduction reaction,  the substance will gain electrons, in other words: "The electrons would be placed on the left side, in the side of the reagents. In an oxidation reaction, the substance will lose electrons, in other words: "The electrons would be placed on the right side, in the side of the products".

With this in mind we will have:

a) Cr+3(aq) + 3e- → Cr (s)(Reduction)

b) Ag(s) → 1e- + Ag+1(ag) (Oxidation)

c) Mn(s) → 5e- + Mn+5(aq) (Oxidation)

d) Sn+2(aq) + 2e- → Sn(s) (Reduction)

I hope it helps!