Le Chatelier's Principle

Increasing the volume of the container will cause the equilibrium to:

• Shift right

• Shift left

• Have no change

• Speed up

Increasing the pressure causes the equilibrium to shift right. Why?

• To increase the pressure more, because there are fewer moles of gas in the products

• Because this makes the equilibrium constant, K, increase

• To reduce the pressure, because there are fewer moles of gas in the products

• To reduce the pressure, because there are more moles of gas in the products

For the reaction...
SO₂ + O₂  <=>  SO₃
If the concentration of SO₂ is increased, the equilibrium position of the reaction will shift ___________.

• to the left

• to the right

• to the left and right 

• neither left nor right

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Consider the following reaction:
2SO_2(g) + O_2(g) <=> 2SO_3(g):  ΔΗ = - 197 kJ mol ^-1
Which of the following will NOT shift the equilibrium position to the right?

• Adding more O₂

• Adding a catalyst

• increasing the pressure

• Lowering the temperature

Tags

NGSS.HS-PS1-4

An understanding of Le Chatelier’s principle is useful in the chemical industry. A prediction that can be made using this principle is the effect of...

• catalysts on the rate of reaction

• catalysts on the position of equilibrium

• changes in temperature on the rate of reaction

• changes in the concentration of reactants on the position of equilibrium

Tags

NGSS.HS-PS1-6

Which of the following statements is true regarding the effect of changing the pressure on a system in dynamic equilibrium?

• Decreasing the pressure may cause the system to favour the reaction that produces fewer moles of gas.

• Increasing the pressure may cause the system to favour the reaction that produces fewer moles of gas

• Increasing the pressure may cause the system to favour the reaction that produces more moles of gas

• Changing the pressure will never have any effect on the position of equilibrium

Which of the following changes would explain the change at time t1 in the graph shown?

• An increase in the volume of the reaction vessel at constant temperature

• A decrease in the volume of the reaction vessel at constant temperature

• Removal of B_(g) at constant volume and temperature

• An increase in temperature at constant volume

Tags

NGSS.HS-PS1-5

The temperature of an equilibrium system with an endothermic forward reaction is increased.

The value of K....

• will increase and the equilibrium position will shift to the right.

• will decrease and the equilibrium position will shift to the right

• will increase and the equilibrium position will shift to the left

• will decrease and the equilibrium position will shift to the left.

The concentration-time graph represents a change to an equilibrium system at time t_1. Which one of the following would account for the changes in concentration at time t₁?

• The addition of X _(aq)

• The removal of Y_(aq)

• An increase in temperature

• A decrease in temperature

Tags

NGSS.HS-PS1-5

Hydrogen is produced on an industrial scale from methane, as follows. If an inert gas is added to an equilibrium system at a constant temperature and a constant volume, the concentration of hydrogen will...

• increase.

• decrease.

• not change.

• decrease then increase.