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Lesson: Le Chatelier's Principle

In this lesson, we will learn how to use Le Chatelier's principle to predict directions of change for equilibria in response to a stimulus.

Worksheet • 18 Questions

Q1:

Ammonia is a weak base that reacts with water according to this equation: Which one of the following, if added to the solution, would increase the proportion of ammonia that is converted to the ammonium ion?

  • A H C l
  • B N a C l
  • C N a O H
  • D N H O H 4
  • E N H C l 4

Q2:

Suppose you wanted to shift the equilibrium position of the reaction 2 N O ( ) N O ( ) 2 2 4 g g in the direction that favors more dimer formation. Which of the following changes in reaction conditions would help achieve that goal?

  • AAn increase in the total pressure of the reaction mixture, with temperature held constant
  • BAn increase in the temperature of the reaction mixture, with total pressure held constant
  • CA simultaneous increase in temperature and increase in pressure
  • DA decrease in the total pressure of the reaction mixture, with temperature held constant

Q3:

Which of the following would decrease the proportion of hydrazine, N H 2 4 , in an equilibrium described by the following equation?

  • ADecrease the pressure
  • BHeat the mixture
  • CAdd N 2
  • DDecrease the volume of the container
  • EAdd H 2

Q4:

Consider the exothermic reaction C O ( ) + 2 H ( ) C H O H ( ) g g g 2 3 at equilibrium at 500 K and 10 bar. Which of the following actions would lead to a decrease in the amount of methanol in the equilibrium reaction mixture?

  • AThe temperature is raised from 500 K to 600 K.
  • BThe pressure is increased from 10 bar to 12 bar.
  • CHydrogen ( H ) 2 gas is added to the mixture at constant pressure.
  • DAn inert (unreactive) gas is pumped into the reaction mixture under constant-volume conditions.

Q5:

Which of the following will increase the percent of N H 3 that is converted to the ammonium ion in water?

  • AAddition of H C l
  • BAddition of N H C l 4
  • CAddition of H O 2
  • DAddition of N a O H

Q6:

In which direction will an increase in temperature shift the position of equilibrium in the following reaction?

  • ATo the right
  • BTo the left
  • CNot enough information has been provided.
  • DNeither: a change in temperature will not change the position of the equilibrium.

Q7:

In which direction will an increase in temperature shift the position of equilibrium in the following reaction?

  • ATo the right
  • BTo the left
  • CNot enough information has been provided.
  • DNeither: a change in temperature will not change the position of the equilibrium.

Q8:

In which direction will a decrease in container volume shift the following equilibrium?

  • ATo the left
  • BTo the right
  • CNot enough information is provided.
  • DNeither: a change in container volume will not change the position of the equilibrium.

Q9:

Which of the following will cause [ H N O ] 2 to decrease in an aqueous solution of K N O 2 ?

  • AAdding N a O H
  • BAdding K N O 2
  • CAdding H N O 2
  • DAdding H C l
  • EAdding N a C l

Q10:

Which of the following will cause [ N O ] 2 – to decrease in an aqueous solution of K N O 2 ?

  • AAdding H C l
  • BAdding K N O 2
  • CAdding H N O 2
  • DAdding N a C l
  • EAdding N a O H

Q11:

In which direction will a decrease in container volume shift the following equilibrium?

  • ANeither: a change in container volume will not change the position of the equilibrium.
  • BTo the right
  • CNot enough information is provided.
  • DTo the left

Q12:

In which direction will a decrease in container volume shift the following equilibrium?

  • ATo the left
  • BTo the right
  • CNot enough information is provided.
  • DNeither: a change in container volume will not change the position of the equilibrium.

Q13:

In which direction will a decrease in container volume shift the following equilibrium?

  • ATo the right
  • BTo the left
  • CNot enough information is provided.
  • DNeither: a change in container volume will not change the position of the equilibrium.

Q14:

Nitrogen and hydrogen react to form ammonia gas with no change in temperature or volume: If hydrogen is added to the system, which of the following is false?

  • A 𝐾 P will increase.
  • BThe position of equilibrium will move to the right.
  • CP( N H 3 ) will increase.
  • DP( H 2 ) will increase.
  • EP( N 2 ) will decrease.

Q15:

A suspension consists of solid silver(I) sulfate and an equilibrium solution of silver(I) and sulfate ions. If more silver(I) sulfate were added to the solution, which of the following effects would be observed?

  • A A g + and S O 4 2 – concentrations would not change.
  • BThe A g + concentration would decrease and the S O 4 2 – concentration would increase.
  • CThe added silver(I) sulfate would dissolve.
  • DThe A g + concentration would increase and the S O 4 2 – concentration would decrease.
  • EAdditional silver(I) sulfate would form and precipitate from solution as A g + ions and S O 4 2 – ions combined.

Q16:

In which direction will an increase in temperature shift the position of equilibrium in the following reaction?

  • ATo the left
  • BTo the right
  • CNot enough information has been provided.
  • DNeither: a change in temperature will not change the position of the equilibrium.

Q17:

How does an increase in temperature affect the equilibrium constant for an exothermic reaction?

  • AIt decreases its value.
  • BIt increases its value.
  • CThere is not enough information provided to answer this question.
  • DIt has no effect on its value.

Q18:

In which direction will an increase in temperature shift the position of equilibrium in the following reaction?

  • ATo the left
  • BTo the right
  • CNot enough information has been provided.
  • DNeither: a change in temperature will not change the position of the equilibrium.
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