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

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.

No concepts available.