I have this question in front of me concerning Methanol (CH3OH) & how geseous methanol is formed via the following thermochemical equation:

CO(g)+2H2(g)¡êCH3OH(g)∆H=-90kJ .

Now, it asks me (explanations should show a clear understanding of how Le Chatelier¡¯s principle applies to the situations described)....

i) The effect that increasing the pressure will have on the equilibrium yield of methanol.

ii) The effect that increasing the temperature will have on the equilibrium yield of methanol.

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

Please can you help me?

All about LeChatelier's Principle.
1. For gases,
a. increased presssure. The reaction will shift toward the side (or direction) that has fewer moles. There are 3 mols on the left and 1 on the right. So the reaction will shift to the right.
b. decreaed pressure. the opposite.

b. The reaction will shift so as to use up the energy from the increase in T. The reaction is exothermic meaning it gives off heat. Therefore, increasing T will cause it to shift to the left.

c.Generally, increasing T causes gaseous molecules to have more energy and that increases the rate of reaction. Notice that the problem doesn't say the forward reaction or the reverse reaction. Increasing T MAY increase both.

I hope this helps. Post any follow up you need.

Sure, I'd be happy to help you understand how Le Chatelier's principle applies to these situations.

i) The effect that increasing the pressure will have on the equilibrium yield of methanol:
According to Le Chatelier's principle, when the pressure is increased, the reaction will shift in the direction that decreases the number of moles of gas. In this case, there are 3 moles of gas on the left side (CO and H2) and 1 mole of gas on the right side (CH3OH). So, increasing the pressure will cause the reaction to shift towards the right, resulting in an increased yield of gaseous methanol.

ii) The effect that increasing the temperature will have on the equilibrium yield of methanol:
Since the reaction is exothermic (it releases heat), increasing the temperature will cause the reaction to shift in the direction that absorbs heat. According to Le Chatelier's principle, this means that increasing the temperature will cause the reaction to shift to the left, resulting in a decreased yield of methanol.

iii) The effect that increasing the temperature will have on the rate of reaction:
Increasing the temperature generally increases the kinetic energy of molecules, which leads to more frequent and energetic collisions between particles. This typically increases the rate of reaction for both the forward and reverse reactions. However, it's important to note that the problem doesn't specify whether it's asking about the rate of the forward reaction or the rate of the reverse reaction. So, in this case, increasing the temperature may increase the rate of both the forward and reverse reactions.

I hope this explanation helps you understand how Le Chatelier's principle applies to these situations. Let me know if you have any further questions!