Chemistry, 15.03.2020 02:21 jerseygirl6167

Consider the following reaction: Mg(s) + ZnSO4(aq) → MgSO4(aq) + Zn(s) Which of the following statements regarding this reaction is correct?
The sulfate ion is reduced.
Zinc is the reducing agent.
Magnesium is neither oxidized nor reduced.
Zinc gains two electrons.
Magnesium is the oxidizing agent.

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Answer from: kleathers97

Zinc gains two electrons.

To find out what's going on with the electrons, we can use oxidation numbers.

Oxidation:- It is the Loss Of Electrons. In this process, the oxidation number of an atom increases. The substance that is oxidized is the reducing agent.

Reduction:-It is the gain Of Electrons. In this process, the oxidation number of an atom decreases. The substance that is reduced is the oxidizing agent.

Reaction:- Mg(s) + ZnSO4(aq) → MgSO4(aq) + Zn(s)

oxidation number:- 0 +2 +2 0

The oxidation number of Zn in the above reaction is decreasing from +2 to 0. Zinc has gained two electrons after losing two positive ions.

The statement (1) that is "sulfate ion is reduced is wrong"because the oxidation numbers of the atoms in SO₄²⁻ have not changed, so the sulfate ion has not been reduced o oxidized.

Zn has gained electrons. It has been reduced, so it is the oxidizing agent. So, statement 2 that is zinc is a reducing agent is wrong.

Statement 3 is wrong. The oxidation number of Mg has increased, so it has been oxidized.

Statement 5 is wrong. Mg has been oxidized, so it is the reducing agent.

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Answer from: BardiFan

Zinc gains two electrons.

Explanation:

We can use oxidation numbers to figure out what is happening with the electrons.

Oxidation is the Loss Of Electrons. It is also an increase in oxidation number. The substance that is oxidized is the reducing agent.

Reduction is the Gain Of Electrons. It is also an decrease in oxidation number. The substance that is reduced is the oxidizing agent.

$\rm \stackrel{\hbox{0}}{\hbox{Mg}} + \stackrel{\hbox{+2}}{\hbox{Zn}}\stackrel{\hbox{+6}}{\hbox{S}}\stackrel{\hbox{-2}}{\hbox{O}}_{4} \,\longrightarrow \, \stackrel{\hbox{+2}}{\hbox{Mg}}\stackrel{\hbox{+6}}{\hbox{S}}\stackrel{\hbox{-2}}{\hbox{O}}_{4} + \stackrel{\hbox{0}}{\hbox{Zn}}$

The oxidation number of Zn decreases from +2 to 0. The zinc has lost two positive charges, so it has gained two electrons.

A is wrong. The oxidation numbers of the atoms in SO₄²⁻ have not changed, so the sulfate ion has not been oxidized or reduced.

B is wrong. Zn has gained electrons. It has been reduced, so it is the oxidizing agent,

C is wrong. The oxidation number of Mg has increased, so it has been oxidized.

E is wrong. Mg has been oxidized, so it is the reducing agent.

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Consider the following reaction: Mg(s) + ZnSO4(aq) → MgSO4(aq) + Zn(s) Which of the following statem...

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