In a reaction at equilibrium, what happens if the pressure is increased?

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Question: In a reaction at equilibrium, what happens if the pressure is increased?

Options:

Correct Answer: Shifts to the side with fewer moles of gas

Solution:

Increasing the pressure will shift the equilibrium position towards the side with fewer moles of gas, according to Le Chatelier\'s Principle.

In a reaction at equilibrium, what happens if the pressure is increased?

In a reaction at equilibrium, what happens if the pressure is increased?

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 gases are involved in the reaction and that they take up space.
Step 3: Recognize that increasing the pressure means there is less space for the gas molecules.
Step 4: According to Le Chatelier's Principle, the system will try to reduce the pressure by favoring the side of the reaction with fewer gas molecules.
Step 5: Identify which side of the reaction has fewer moles of gas and understand that the equilibrium will shift towards that side.

Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the system will adjust to counteract that change and restore a new equilibrium.
Equilibrium Position – The state in a chemical reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.
Moles of Gas – In reactions involving gases, the number of moles on each side of the equation can affect how the equilibrium shifts when pressure changes.