What products should be formed when the following reac-tants are electrolyzed in a cell having inert electrodes? Account for any differences. (b) Aqueous KCl

Verified step by step guidance

1. Identify the components present in the aqueous KCl solution: K^+, Cl^-, H_2O.
2. Determine the possible reactions at the anode (oxidation site): Cl^- can be oxidized to Cl_2 gas, and water can be oxidized to O_2 gas.
3. Determine the possible reactions at the cathode (reduction site): K^+ can be reduced to K metal, and water can be reduced to H_2 gas.
4. Compare the standard electrode potentials to determine which reactions are more favorable: Cl^- oxidation vs. water oxidation, and K^+ reduction vs. water reduction.
5. Conclude the most likely products based on the favorable reactions: Cl_2 gas at the anode and H_2 gas at the cathode.

Key Concepts

Electrolysis

Electrolysis is a chemical process that uses electrical energy to drive a non-spontaneous reaction. In an electrolytic cell, an electric current is passed through an electrolyte, causing the decomposition of the compound into its constituent ions. This process occurs at inert electrodes, which do not participate in the reaction but facilitate the transfer of electrons.

Ionic Compounds in Aqueous Solution

When ionic compounds like KCl are dissolved in water, they dissociate into their respective ions (K⁺ and Cl⁻). In electrolysis, these ions migrate towards the electrodes: cations move towards the cathode (negative electrode) and anions towards the anode (positive electrode). The behavior of these ions during electrolysis is crucial for predicting the products formed.

Electrode Reactions

At the electrodes during electrolysis, specific reactions occur based on the ions present and their standard electrode potentials. At the cathode, reduction occurs, typically involving the gain of electrons by cations, while at the anode, oxidation occurs, often involving the loss of electrons by anions. The products formed depend on the nature of the ions and the conditions of the electrolysis.