Methanol is manufactured by the below catalyzed reation using ZnO/Chromate.

CO + 2H2 --> CH3OH deltaH -91kJ
Does the amount of methanol increase, decrease, or remain the same when an equilibrium mixture of reactants and products is subjected to the following changes?
A. the temp increases--decreased
B. the volume is dercreased -increased
C. CO is added--increased
D. the catalysts ZnO/Chromate is removed--no change.
E. Methanol is added? i think it will decrease but just need to check my answer.

A correct

B correct
C correct
D correct
E correct

thank you so much

i have another chemistry question posted farther down can u help me out a bit on that one?

To determine how the amount of methanol changes when the equilibrium mixture of reactants and products is subjected to different changes, we need to apply Le Chatelier's principle. This principle states that a system at equilibrium will adjust itself to counteract any changes imposed upon it.

A. When the temperature increases:
According to the given reaction, the formation of methanol is exothermic (delta H = -91 kJ). Increasing the temperature would shift the equilibrium in the reverse direction to counteract the increase in temperature. Thus, the amount of methanol would decrease.

B. When the volume is decreased:
Decreasing the volume would increase the pressure of the system. As the reaction involves the formation of two moles of gas (CO + 2H2), the equilibrium would shift in the direction that minimizes the number of moles of gas to counteract the pressure increase. Since the formation of methanol is associated with a decrease in the number of gas molecules, the amount of methanol would increase.

C. When CO is added:
Adding more CO to the system would increase the concentration of reactants. According to Le Chatelier's principle, the equilibrium would shift in the direction that minimizes the effect of the increase in reactant concentration. Therefore, the amount of methanol would increase.

D. When the catalyst ZnO/Chromate is removed:
The catalyst does not participate in the chemical reaction itself. Its purpose is to speed up the reaction without being consumed. Thus, removing the catalyst would not have a significant effect on the equilibrium position or the amount of methanol.

E. When methanol is added:
Adding more methanol would increase the concentration of the product. As per Le Chatelier's principle, the equilibrium would shift in the direction that counteracts the effect of the added product. Therefore, the amount of methanol would decrease.

In summary:
A. The amount of methanol decreases when the temperature increases.
B. The amount of methanol increases when the volume is decreased.
C. The amount of methanol increases when CO is added.
D. The amount of methanol remains the same when the catalyst is removed.
E. The amount of methanol decreases when methanol is added.