Lesson Worksheet: Le Chatelier’s Principle Chemistry • 10th Grade
In this worksheet, we will practice explaining the effect of changing the temperature, concentration, or pressure on an equilibrium according to Le Chatelier’s principle.
Q1:
In which of the following gas-phase reactions could the equilibrium yield be increased by increasing temperature or decreasing pressure?
- A
- B
- C
- D
- E
Q2:
In which of the following gas-phase reactions could the equilibrium yield be increased by increasing either temperature or pressure?
- A
- B
- C
- D
- E
Q3:
Molecules and react exothermically and reversibly to produce a third molecule , as shown by the equation.
A box contains five molecules each of , , and at equilibrium, as shown. The temperature inside the box is , and the pressure is 1 bar.
The temperature of the box changes to , and the box expands to maintain a pressure of 1 bar. Which of the following diagrams represents the box at equilibrium under these conditions?
- A
- B
- C
- D
- E
The volume of the box increases at a fixed temperature of . Which of the following diagrams represents the box at equilibrium under these conditions?
- A
- B
- C
- D
- E
At a fixed temperature of , the concentration of is increased and the box changes in volume to maintain a pressure of 1 bar. Which of the following diagrams represents the box at equilibrium under these conditions?
- A
- B
- C
- D
- E
At a fixed temperature of , the concentration of is decreased and the box changes in volume to maintain a pressure of 1 bar. Which of the following diagrams represents the box at equilibrium under these conditions?
- A
- B
- C
- D
- E
Q4:
The following reaction is part of the Ostwald process that produces nitric acid:
Which of the following statements explains why the percentage of produced may decrease as the pressure increases?
- AIncreasing the pressure moves the equilibrium to the right.
- BThe forward reaction is favored by an increase in pressure.
- CThe total volume of gas increases for the backward reaction.
- DFewer moles of gas are on the reactant’s side.
Q5:
Consider the following equation: What effect will increasing the pressure have on the position of the equilibrium?
- AThe equilibrium will move to the right.
- BThe equilibrium will not move.
- CThe equilibrium will move to the left.
Q6:
Sulfur trioxide is produced as part of the process of manufacturing sulfuric acid as shown: What effect will adding more oxygen have on the position of the equilibrium?
- AThe equilibrium will not move.
- BThe equilibrium will move to the right.
- CThe equilibrium will move to the left.
Q7:
The industrial production of ammonia uses nitrogen and hydrogen:
What effect will increasing the pressure have on the position of the equilibrium?
- AThe equilibrium will move to the left.
- BThe equilibrium will not move.
- CThe equilibrium will move to the right.
Q8:
The industrial production of ethanol uses ethene gas and steam, as shown:
Considering that the forward reaction is exothermic, what effect will increasing the temperature have on the position of the equilibrium?
- AThe equilibrium will not move.
- BThe equilibrium will move to the left.
- CThe equilibrium will move to the right.
Q9:
Which of the following statements best defines Le Chatelier’s principle?
- AIf conditions change in a dynamic equilibrium, the position of the equilibrium moves to increase the change.
- BIf a chemical reaction is at equilibrium and experiences a change in pressure, temperature, or concentration of products or reactants, the equilibrium shifts in the opposite direction to increase the rate of reaction.
- CIf a change occurs to an equilibrium mixture, the system will tend to adjust itself so as to cancel out, as far as possible, the effect of that change.
- DChanges in the temperature and pressure in a system will result in changes to the system in order to achieve a new equilibrium state.
- EWhen a system at equilibrium is subjected to changes in concentration or volume, the system shifts to a new equilibrium to counteract the applied change.
Q10:
Iodine trichloride is a bright yellow interhalogen compound formed in the following reaction: What effect will removing chlorine have on the position of the equilibrium?
- AThe equilibrium will move to the right.
- BThe equilibrium will move to the left.
- CThe equilibrium will not move.
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