In a reaction at equilibrium, what effect does increasing the pressure have if the number of moles of gas on the reactant side is greater than that on the product side?
Practice Questions
1 question
Q1
In a reaction at equilibrium, what effect does increasing the pressure have if the number of moles of gas on the reactant side is greater than that on the product side?
Shifts to the right
Shifts to the left
No effect
Reaction rate decreases
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 effect does increasing the pressure have if the number of moles of gas on the reactant side is greater than that 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: 7
Step 1: Understand what equilibrium means. It is a state where the forward and reverse reactions happen at the same rate.
Step 2: Know that gases occupy space and pressure is related to the number of gas molecules.
Step 3: Identify the sides of the reaction: the reactants (left side) and the products (right side).
Step 4: Count the number of moles of gas on both sides of the reaction. The reactants have more moles than the products.
Step 5: Remember Le Chatelier's Principle, which states that if you change the conditions of a system at equilibrium, the system will adjust to counteract that change.
Step 6: When you increase the pressure, the system will try to reduce the pressure by favoring the side with fewer moles of gas.
Step 7: Since the product side has fewer moles of gas, the equilibrium will shift to the right, favoring the products.
