In a reaction at equilibrium, what happens if the pressure is increased for a reaction with fewer moles of gas on the product side?
Practice Questions
1 question
Q1
In a reaction at equilibrium, what happens if the pressure is increased for a reaction with fewer moles of gas on the product side?
Shifts equilibrium to the right
Shifts equilibrium to the left
No effect on equilibrium
Increases the rate of reaction
Increasing the pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas, according to Le Chatelier's Principle.
Questions & Step-by-step Solutions
1 item
Q
Q: In a reaction at equilibrium, what happens if the pressure is increased for a reaction with fewer moles of gas on the product side?
Solution: Increasing the pressure will shift the equilibrium to the right, favoring the side with fewer moles of gas, according to Le Chatelier's Principle.
Steps: 6
Step 1: Understand that a chemical reaction can reach a state called equilibrium, where the forward and reverse reactions happen at the same rate.
Step 2: Know that in a reaction, there are reactants (starting materials) and products (end results).
Step 3: Recognize that gases take up space, and the number of gas molecules can affect pressure.
Step 4: Learn about Le Chatelier's Principle, which states that if you change the conditions of a reaction at equilibrium, the system will adjust to counteract that change.
Step 5: If you increase the pressure in a reaction, the equilibrium will shift to the side with fewer gas molecules to reduce the pressure.
Step 6: In this case, since the product side has fewer moles of gas, the equilibrium will shift to the right, favoring the products.
