MgSO4+2K yields K2SO4+Mg. Would the oxidation reaction be 2K yields K2+e-2?And would the reduction be MG+e- yields Mg? Thanks.

The oxidation reaction would be

K yields K+ + e-

(When adding the reduction-half and oxidation-half, the oxidation equation will be multiplied by 2.)

Hope this helps.

The reduction equation is

Mg + 2e ==> Mg
Note the 2e, not 1e.

The given reaction is:

MgSO4 + 2K → K2SO4 + Mg

To identify the oxidation and reduction reactions, we need to assign oxidation numbers to each element involved:

In MgSO4:
- Oxygen (O) always has an oxidation state of -2, so in MgSO4, the total oxidation state of oxygen is (-2) * 4 = -8.
- The sum of oxidation numbers in a compound is always zero, so we can assign magnesium (Mg) an oxidation state of +2 to balance out the negative charge.
- Sulfur (S) will have an oxidation state of +6. (This is because the sum of oxidation numbers in a compound is always zero, and sulfur must have an oxidation state of +6 to cancel out the -8 from oxygen.)

In K2SO4:
- Since potassium (K) is an alkali metal, its oxidation state is +1.
- We already know the oxidation state of oxygen in compounds is usually -2.
- To balance out the charges, the oxidation state of sulfur must be +6. (Since there are two potassium atoms each with an oxidation state of +1, the total positive charge is +2. The oxidation state of sulfur must be +6 to balance this out.)

Based on the changes in oxidation states, we can identify the oxidation and reduction reactions:

Oxidation Half-Reaction: 2K → 2K+ + 2e-
Reduction Half-Reaction: Mg2+ + 2e- → Mg

Please note that the oxidation state of magnesium changes from 0 to +2 to form Mg2+ in the reduction half-reaction.

To determine the oxidation and reduction reactions in a chemical equation, we need to identify the changes in the oxidation states of the elements involved.

In the given equation:
MgSO4 + 2K → K2SO4 + Mg

The oxidation state of K (potassium) is +1 in both K and K2SO4. Therefore, there is no change in the oxidation state of potassium, and it is not involved in any redox reaction.

On the other hand, the oxidation state of Mg (magnesium) changes from 0 to +2. This means that Mg has been oxidized since its oxidation state has increased.

The half-reaction for oxidation can be represented as:
Mg → Mg2+ + 2e-

As for the reduction half-reaction, the oxidation state of S (sulfur) changes from +6 to +4. This indicates that S has been reduced since its oxidation state has decreased.

The half-reaction for reduction can be represented as:
SO4^2- + 8e- → SO4^2- + 4e-

Therefore, the oxidation reaction would be: Mg → Mg2+ + 2e-
And the reduction reaction would be: SO4^2- + 8e- → SO4^2- + 4e-