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.
