Question

A zinc-copper cell is constructed: Zn | Zn2+ (1M) || Cu2+ (1M) | Cu. What occurs to the mass of the copper electrode as the reaction proceeds? (Zinc is above copper in the activity series of metals.)

It decreases.
It remains the same.
It increases.

Answer 1

As the reaction proceed the mass of the Copper electrode will increase.

Answer 2

The mass of the copper electrode increases as the reaction proceeds

Explanation:

The representation of electrochemical cell is given by writing the anode on left hand side followed by its ion with its molar concentration. It is followed by a salt bridge.Then the cathodic ion with its molar concentration is written and then the cathode.

Oxidation occurs at anode. Oxidation reaction is defined as the reaction in which a substance looses its electrons. Zinc loses electrons and convert to zinc ions and thus the mass keeps on decreasing with time.

Anode : $Zn\rightarrow Zn^{2+}+2e^-$

Reduction occurs at cathode. Reduction reaction is defined as the reaction in which a substance gains electrons. Copper gains electrons and convert copper ions from solution to copper and thus keeps depositing and mass keeps on increasing with time.

$Cu^{2+}+2e^-\rightarrow Cu$

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