Question

Look at the diagram of an electrochemical cell below.

Answer 1

Answer is: charges are balanced during redox.
1) False. Electrons are produced on zinc rod (Zn → Zn²⁺ + 2e⁻)
2) False. Electrons flow from anode (negative electrode) to cathode (positive electrode).
3) False.Oxidation occurs at the zinc electrolyte (Zn → Zn²⁺).

Answer 2

Answer : The correct option is, Charges are balanced during the redox reaction.

Explanation :

Electrochemical cell : It is a device a that is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy.

The redox reaction occurs between the zinc and copper sulfate.

In the electrochemical cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

The balanced two-half reactions will be,

Oxidation half reaction : $Zn(s)\rightarrow Zn^{2+}(aq)+2e^-$

Reduction half reaction : $Cu^{2+}(aq)+2e^-\rightarrow Cu(s)$

Thus the overall reaction will be,

$Zn(s)+Cu^{2+}(aq)\rightarrow Zn^{2+}(aq)+Cu(s)$

From the given options, we conclude that the options, charges are balanced during the redox reaction are correct statement. While the other statements are wrong. The correct statements will be :

The electrons are produced at zinc electrode.

The electrons flow from anode to cathode.

Oxidation occurs at the zinc electrolyte.

Reduction occurs at the copper electrolyte.

Therefore, the correct option is, Charges are balanced during the redox reaction.