How does increasing pressure affect the equilibrium of the reaction CO(g) + 2H2(g) ⇌ CH3OH(g)?
Understand the Problem
The question is asking about the effect of changing pressure on the equilibrium position of a chemical reaction involving gases. Specifically, it's inquiring whether increasing the pressure will shift the equilibrium towards the production of methanol (CH3OH) or not, given that there are three moles of gas reactants (CO and H2) and only one mole of gas product (CH3OH). This invokes the principles of Le Chatelier's principle.
Answer
Increasing pressure shifts equilibrium towards CH3OH, increasing its yield.
Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, which in this case is the right side, increasing the yield of methanol.
Answer for screen readers
Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, which in this case is the right side, increasing the yield of methanol.
More Information
More pressure favors the production of methanol because it reduces the number of moles of gas within the system, thus adhering to Le Chatelier's Principle.
Tips
A common mistake is forgetting to count the number of moles of gas on each side of the equilibrium reaction before predicting the shift.
Sources
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