In a reaction at equilibrium, what effect does increasing the pressure have if t
Practice Questions
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 on the product side?
Shifts to the right
Shifts to the left
No effect
Reaction stops
Questions & Step-by-Step Solutions
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 on the product side?
Step 1: Understand what equilibrium means. It is a state where the forward and reverse reactions occur at the same rate.
Step 2: Identify the sides of the reaction. The reactant side has more moles of gas than the product side.
Step 3: Know that increasing pressure affects gases. It pushes the reaction towards the side with fewer gas moles.
Step 4: Since the reactant side has more moles, increasing pressure will shift the equilibrium to the right, towards the product side.
Step 5: Conclude that increasing pressure favors the side with fewer moles of gas, which is the product side in this case.
