GCSE Chemistry - Le Chatelier's Principle #50 (Higher Tier)

The video tutorial explains the position of equilibrium in reversible reactions and how it is influenced by changes in temperature, pressure, and concentration. It introduces Le Chatelier's principle, which predicts how equilibrium shifts to counteract changes in conditions. The video uses the example of ammonia production to illustrate how equilibrium moves in response to temperature changes, pressure variations, and concentration adjustments.

What does Le Chatelier's principle help us predict in a reversible reaction?

• The speed of the reaction

• The shift in equilibrium position due to changes in conditions

• The color change of the reactants

• The formation of new compounds

In the production of ammonia, what happens to the equilibrium position when the temperature is decreased?

• It shifts randomly

• It shifts to the right, favoring ammonia

• It shifts to the left, favoring nitrogen and hydrogen

• It remains unchanged

How does increasing the temperature affect the equilibrium in an exothermic reaction?

• Equilibrium shifts to the right

• Equilibrium shifts to the left

• Equilibrium shifts to both sides equally

• Equilibrium remains unchanged

What is the effect of increasing pressure on the equilibrium position in a reaction with more molecules on the left side?

• Equilibrium shifts to the left

• Equilibrium shifts to the right

• Equilibrium remains unchanged

• Equilibrium shifts to both sides equally

If more nitrogen is added to a sealed container, how does the equilibrium shift?

• Equilibrium remains unchanged

• Equilibrium shifts to the right

• Equilibrium shifts to the left

• Equilibrium shifts to both sides equally