Consider the following reaction: Mn(s) + CuSO4(aq) → MnSO4(aq) + Cu(s) Which of the following statements regarding this reaction is correct?

The sulfate ion is oxidized.

Each copper gains two electrons.

Manganese is the oxidizing agent.

Manganese is neither oxidized nor reduced.

Copper is the reducing agent.
Please answer quickly

Each copper gains two electrons

Explanation:

Oxidizing agents:

Oxidizing agents oxidize the other elements and itself gets reduced.

Reducing agents:

Reducing agents reduced the other element are it self gets oxidized.

Chemical equation:

CuSO₄ + Mn   →  MnSO₄  + Cu

This is single replacement reaction. Manganese replace the copper and react with sulfate to form copper sulfate.

Copper gains two electrons and gets reduced. The oxidation state of copper on left side is +2 while on right side its 0 so it gain two electrons and gets reduced.

while oxidation state of manganese on left side is 0 while on right side its +2. It means Mn lose to electrons and gets oxidized.

So  copper is oxidizing agent while manganese is reducing agent.

while the oxidation state of sulfate is not changed.

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explanation:

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it is called acid bonding