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In a reaction at equilibrium, what effect does increasing the pressure have if t

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Question: 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?

Options:

  1. Shifts to the right
  2. Shifts to the left
  3. No effect
  4. Reaction rate decreases

Correct Answer: Shifts 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 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 that on the product side?
  1. Shifts to the right
  2. Shifts to the left
  3. No effect
  4. Reaction rate decreases

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 that on the product side?
  • 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.
  • 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.
  • Mole Count in Gases – Recognizing the significance of the number of moles of gas on each side of the reaction in determining the direction of the shift.
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