For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure?
Practice Questions
1 question
Q1
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure?
Shifts equilibrium to the left
Shifts equilibrium to the right
No effect on equilibrium
Increases the temperature
Increasing the pressure will shift the equilibrium to the right, favoring the production of SO3, as it has fewer moles of gas (3 moles to 2 moles).
Questions & Step-by-step Solutions
1 item
Q
Q: For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure?
Solution: Increasing the pressure will shift the equilibrium to the right, favoring the production of SO3, as it has fewer moles of gas (3 moles to 2 moles).
Steps: 7
Step 1: Identify the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g).
Step 2: Count the number of gas moles on each side of the reaction.
Step 3: On the left side (reactants), there are 2 moles of SO2 and 1 mole of O2, totaling 3 moles.
Step 4: On the right side (products), there are 2 moles of SO3.
Step 5: Compare the total moles: 3 moles (reactants) vs. 2 moles (products).
Step 6: Understand that increasing pressure favors the side with fewer moles of gas.
Step 7: Conclude that increasing the pressure will shift the equilibrium to the right, producing more SO3.
