Equilibrium:

The following question(s) refer to the equilibrium in which all reactants and products are gases:

[tex]\[ CH_4 + H_2O \rightleftarrows CH_3OH + H_2 + \text{heat} \][/tex]

Indicate the effect of the changing condition on the position of equilibrium.

Cool the mixture.



Answer :

Alright, let's consider the equilibrium reaction:

[tex]\[ \text{CH}_4 + \text{H}_2\text{O} \rightleftharpoons \text{CH}_3\text{OH} + \text{H}_2 + \text{heat} \][/tex]

This reaction is exothermic, meaning it produces heat as a product. Now, we want to determine the effect on the position of equilibrium when the mixture is cooled.

1. Identify the Nature of the Reaction: As stated, the reaction is exothermic (it produces heat).

2. Application of Le Chatelier's Principle: According to Le Chatelier's Principle, if a disturbance is applied to a system at equilibrium, the system will adjust itself to counteract the disturbance and re-establish equilibrium.

3. Determine the Disturbance: In this scenario, cooling the mixture is the disturbance. Cooling removes heat from the system.

4. Predict the Shift in Equilibrium: To counteract the loss of heat (cooling), the system will shift in a direction that produces more heat. In an exothermic reaction, heat is produced on the right side (products side) of the equilibrium.

5. Shift Direction: Thus, to produce more heat, the equilibrium will shift towards the right side (products side).

6. Conclusion: Cooling the mixture will cause the equilibrium to shift to the right side, favoring the production of the products (CH₃OH and H₂).

So, to summarize, cooling the mixture will shift the equilibrium to the right.