Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Chapter
Reversible Reactions and Equilibria
144 practice questions
Topics covered
- Reversibility and dynamic equilibria19 practice questions
- Reversible reactions in a sealed container18 practice questions
- The position of equilibrium20 practice questions
- Changing the pressure19 practice questions
- Changing the temperature19 practice questions
- Adding a catalyst19 practice questions
- The effect of concentration19 practice questions
Practice questions
61–70 of 144
Question 61
2 marks · Easy
Answer and see the solution →Consider the following equilibrium:
Explain, with a reason, what would happen to the position of equilibrium if the pressure is decreased.
Question 62
3 marks · Easy
Answer and see the solution →For the following equilibrium:
A chemist measured the percentage of E(g), F(g), and G(g) at equilibrium under different pressure conditions. Use the data to answer the questions.
Condition % E(g) % F(g) % G(g) Low pressure 30 30 40 High pressure 25 25 50 (a)[1 mark]State the number of gaseous molecules on each side of the equation.
(b)[1 mark]Describe the effect of increasing the pressure on the position of equilibrium, using the data.
(c)[1 mark]Explain your answer to part (b).
Question 63
1 mark · Easy
Answer and see the solution →The following reaction is at equilibrium in a container:
If the pressure is increased, which direction will the equilibrium shift?
Question 64
3 marks · Easy
Answer and see the solution →Consider the following equilibrium, which is carried out in a sealed container:
(a)[1 mark]State the number of gas molecules on the left and the right side of the equation.
(b)[1 mark]State what will happen to the equilibrium position if the pressure is increased.
(c)[1 mark]Give a reason for your answer to part (b).
Question 65
2 marks · Easy
Answer and see the solution →The following reaction is at equilibrium at 400 K:
If the total pressure is doubled, predict the effect on the amount of A(g) formed at equilibrium. Show your reasoning.
(a)[1 mark]Calculate the number of gaseous molecules on each side of the equation.
(b)[1 mark]State whether the amount of A(g) at equilibrium will increase, decrease, or stay the same. Explain your answer.
Question 66
2 marks · Normal
Answer and see the solution →State why changing the pressure affects only equilibria involving gases, and only when the numbers of gaseous molecules on each side of the equation are different.
Question 67
4 marks · Normal
Answer and see the solution →The following reaction takes place in a closed container:
(a)[1 mark]State the total number of moles of gas on each side of this equation.
(b)[3 marks]The pressure of the system is increased. Predict and explain the direction in which the equilibrium will shift.
Question 68
3 marks · Normal
Answer and see the solution →The reaction below is allowed to reach equilibrium in a sealed container:
Explain, using the number of moles of gas, what will happen to the position of equilibrium if the pressure is decreased.
Question 69
4 marks · Normal
Answer and see the solution →Consider the following data collected for this equilibrium reaction:
Condition % M(g) % N(g) % Q(g) Low pressure 40 40 20 High pressure 45 45 10 (a)[1 mark]What is the total number of moles of gas on each side of the equation?
(b)[2 marks]Describe the effect that increasing pressure has on the amounts of M(g), N(g), and Q(g).
(c)[1 mark]Explain your answer to (b) in terms of the number of gas molecules.
Question 70
1 mark · Normal
Answer and check →Consider the following equilibrium:
What will happen to the position of equilibrium if the pressure is increased?
- A.It shifts to the left (towards \ce{F2})
- B.It shifts to the right (towards \ce{F})
- C.No effect
- D.It shifts to both sides equally