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

Question

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.