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

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Question: In a reaction at equilibrium, what happens if the pressure is increased for a reaction with fewer moles of gas on the product side?

Options:

Correct Answer: Shifts equilibrium to the right

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.

In a reaction at equilibrium, what happens if the pressure is increased for a reaction with fewer moles of gas on the product side?

In a reaction at equilibrium, what happens if the pressure is increased for a reaction with fewer moles of gas on the product side?

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.

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 Shift – Understanding how changes in conditions (like pressure) affect the position of equilibrium in a chemical reaction.
Moles of Gas – Recognizing the significance of the number of moles of gas on each side of a reaction when predicting the effect of pressure changes.