Write the net ionic equations and determine the standard potentials for the reaction of copper or zinc

The complete question is "Write the net ionic equations and determine the standard potentials for the reaction of copper or zinc with Tin (IV)"

1) Reaction of copper with Tin (IV)

Tin is in highest oxidation state which is +4. It cannot be oxidized further.

Therefore it will undergo reduction. The reduction half reaction can be written as

Using standard reduction potential table, we can find E⁰ red for this reaction.

E⁰ red = 0.15 V

Copper undergoes oxidation. The oxidation half reaction can be written as follows.

Standard reduction potential of Cu from the table is 0.34 V. But since this is an oxidation reaction we will reverse the sign of E⁰ to get E⁰ ox.

E⁰ox = -0.34 V

In order to write the net ionic equation, we will combine the above half reactions.

The net ionic equation is

Standard cell potential for this reaction is calculated as

E^{0}_{cell}= -0.19V

Cell potential for the reaction of copper with tin (IV) is -0.19 V

2) Reaction of zinc with tin (IV)

The reduction half reaction can be written as

As discussed in part 1 , E⁰red = 0.15 V

Zinc undergoes oxidation. The oxidation half reaction can be written as

Standard reduction potential of zinc from the table is -0.76 V.

Since we have an oxidation reaction here, we will reverse the sign to get E⁰ox

E⁰ox = 0.76 V

The net cell reaction is

Standard cell potential can be calculated as

The standard potential for the reaction of zinc with tin (IV) is 0.91 V

alchemy hadn't scientific methods of study, appeal to mysticism and fantasy, the knowledge of chemistry and physics were modest at that time.

alchemy was - but as new rules were discovered it either changed into chemistry or it became "unscientific".