Question

During the electrolysis of aqueous KCl solution using inert electrodes, gaseous hydrogen is evolved at one electrode and gaseous chlorine at the other electrode. The solution around the electrode at which hydrogen gas is evolved becomes basic as the electrolysis proceeds. Which of the following responses describe or are applicable to the cathode and the reaction that occurs at the cathode? Select all that apply.

a. The positive electrode
b. The negative electrode
c. 2Cl– ⇌ Cl2 + 2e–
d. Cl2 + 2e– ⇌ 2Cl–
e. 2H2O ⇌ O2 + 4H+ + 4e–
f. 2H2O + 2e– ⇌ H2 + 2OH–
g. Electrons flow from the electrode to the external circuit
h. Electrons flow into the electrode from the external circuit
i. Oxidation
j. Reduction

Answer 1

Following is the correct description of the problem.

Step-by-step explanation:

• Electricity flows through all the cathode(from the anode via the outer wire).
• Reduction takes place at the cathode (electron benefit).
• The cathode electrode seems to be positive as well as the anode negative.
• 2H₂O + 2e → H₂ + 2OH⁻ (In this, there's really a rivalry between potassium as well as hydrogen ions, but mostly because hydrogen requires potential benefits for reduction or potassium requires negative ability to reduce hydrogen to hydrogen throughout the best possible method. Potassium oxidizes stronger than its ions).