For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is
Practice Questions
Q1
For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is increased?
Equilibrium shifts to the left
Equilibrium shifts to the right
No change in equilibrium
Equilibrium constant increases
Questions & Step-by-Step Solutions
For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is increased?
Step 1: Identify the reaction: CO(g) + 2H2(g) ⇌ CH3OH(g).
Step 2: Count the number of gas moles on each side of the reaction.
Step 3: On the left side (reactants), there are 3 moles: 1 mole of CO and 2 moles of H2.
Step 4: On the right side (products), there is 1 mole of CH3OH.
Step 5: Compare the total moles: Left side has 3 moles, right side has 1 mole.
Step 6: Understand that increasing pressure in a reaction favors the side with fewer moles of gas.
Step 7: Since the right side has fewer moles (1 mole), the equilibrium will shift to the right.
Le Chatelier's Principle – This principle states that if an external change is applied to a system at equilibrium, the system will adjust to counteract that change and restore a new equilibrium.
Mole Count in Gaseous Reactions – Understanding how to count the number of moles of gas on each side of a chemical equation is crucial for predicting the direction of the shift in equilibrium when pressure changes.
