State the Le Chatelier's principle and explain the following

i) The effect that incresing the pressure will have on the eaualibrium yield of methanol

ii) The effect of increasing the temperature will have on the equalibrium yeild of methanol

iii) The effect of the increasing temperature will have on the rate of reaction.

where appropriate, your explanations should show a clear understanding of how the Le Chateliers principle applies to the situations decribed.

See my response to bex just below your post.

Le Chatelier's principle states that when a system in equilibrium is subjected to a change, it will adjust to counteract the change and maintain equilibrium.

i) Increasing the pressure: In the production of methanol, the reaction involves the conversion of carbon monoxide and hydrogen gas into methanol. According to Le Chatelier's principle, increasing the pressure will cause the system to shift in the direction that reduces the total number of gas molecules. As the forward reaction produces one mole of methanol gas, while the reactants produce two moles of gas (CO and H2), increasing the pressure will favor the forward reaction to reduce the number of gas molecules. Therefore, increasing the pressure will increase the equilibrium yield of methanol.

ii) Increasing the temperature: In the methanol production reaction, it is an exothermic reaction, meaning it releases heat. According to Le Chatelier's principle, increasing the temperature will cause the system to shift in the direction that absorbs heat. To counteract the increase in temperature, the equilibrium will shift in the endothermic direction, which is the reverse reaction. As a result, the equilibrium yield of methanol will decrease since it is favored at lower temperatures.

iii) Increasing the temperature's effect on the rate of reaction: Le Chatelier's principle does not specifically apply to the rate of reaction but rather to the equilibrium position. However, increasing the temperature generally increases the rate of reaction according to the Arrhenius equation. As the temperature increases, the kinetic energy of reacting particles increases, leading to more successful collisions and a higher rate of reaction. This effect occurs regardless of the equilibrium position.