Question

Consider the following reaction taking place in a voltaic cell:

Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)

What will happen to the Cu?

a. Cu is reduced at the anode and Ag+ is oxidized at the cathode.
b. Cu is oxidized at the cathode and Ag+ is reduced at the anode.
c. Cu is oxidized at the anode and Ag+ is reduced at the cathode.
d. Cu is reduced at the cathode and Ag+ is oxidized at the anode.

Answer 1

Option C. Cu is oxidized at the anode and Ag+ is reduced at the cathode.

Step-by-step explanation:

The reaction that is taking place in the voltaic cell is:

Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

A voltaic cell is an electrochemical cell that uses spontaneous redox reactions, like the above, to generate electricity.

In the rection above, the electrode of the anode is Cu, and the electrode of the cathode is Ag. In the cell, the solution of Ag⁺ produces the oxidation of the Cu(s) which results in Cu²⁺ and Ag(s) (since the Ag⁺ is being reduced). In a voltaic cell, the anode is the electrode at which the oxidation reaction occurs and the cathode is the electrode at which the reduction reaction takes place.

The redox reactions in this system release energy, so a wire connects the two reactions and allows electrons to flow from one side to the other, forming the Voltaic (or Galvanic) Cell.

From all of the above, the correct option is c: Cu is oxidized at the anode, and Ag+ is reduced at the cathode.

I hope it helps you!