Question

Consider the following reaction: Mn(s) + CuSO4(aq) → MnSO4(aq) + Cu(s) Which of the following statements regarding this reaction is correct?
Manganese is neither oxidized nor reduced.
Copper is the reducing agent.
Each copper gains two electrons.
Manganese is the oxidizing agent.
The sulfate ion is oxidized.
I need help asap please and thank you

Answer 1

Answer:

Each copper gains two electrons

Explanation:

Chemical equation:

CuSO₄(aq) + Mn(s)   →  MnSO₄(aq)  + Cu(s)

This is single replacement reaction. The reactivity of manganese is higher than copper that's why 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.

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.