Question

Which of the following will favor CH₄ at equilibrium?

- Adding more C to the reaction mixture
- Adding a catalyst to the reaction mixture
- Lowering the volume of the reaction mixture
- Adding neon gas to the reaction mixture
- Adding more H₂ to the reaction mixture
- Raising the temperature of the reaction mixture

Answer 1

To favor the formation of CH₄ at equilibrium, adding more C and H₂ to the reaction mixture and lowering the volume will help, while adding a catalyst, neon gas, and raising the temperature will not.

Step-by-step explanation:

To favor the formation of CH₄ at equilibrium, the following factors can be considered:

• Adding more C to the reaction mixture: This will shift the equilibrium towards the formation of CH₄ since there will be more reactant available.
• Adding a catalyst to the reaction mixture: A catalyst does not affect the equilibrium position but increases the rate of reaction. It will not specifically favor CH₄ formation.
• Lowering the volume of the reaction mixture: Decreasing the volume will increase the pressure, favoring the side with fewer moles of gas. In this case, it will favor the formation of CH₄.

• Adding neon gas to the reaction mixture: Neon gas is inert and does not participate in the reaction. Therefore, it will not affect the equilibrium position.
• Adding more H₂ to the reaction mixture: Increasing the concentration of H₂ will shift the equilibrium towards the formation of CH₄ since there will be more reactant available.
• Raising the temperature of the reaction mixture: Increasing the temperature will favor the endothermic reaction and shift the equilibrium towards the reactant side. Therefore, it will not favor the formation of CH₄.