Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Section
Changing the pressure
19 practice questions
Practice questions
11–19 of 19
Question 11
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 12
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 13
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
Question 14
2 marks · Normal
Answer and see the solution →For equilibria involving only solids and liquids, changing the pressure has very little effect. Give two reasons why.
Question 15
4 marks · Normal
Answer and see the solution →Carbon monoxide and hydrogen react according to the following equation:
(a)[1 mark]How many moles of gaseous molecules are there on each side of the equation?
(b)[3 marks]If the pressure is increased, what happens to the position of equilibrium? Explain your answer.
Question 16
3 marks · Normal
Answer and see the solution →The following reaction is allowed to reach equilibrium in a sealed container:
The number of gaseous molecules on each side of the equation is different.
Explain, with calculations, why increasing the pressure will affect this equilibrium, and state which side the equilibrium will shift towards. Use the number of moles of gas in your answer.
Question 17
2 marks · Hard
Answer and see the solution →Consider the following reversible reaction, which takes place in a sealed vessel at constant temperature:
Explain why changing the pressure will or will not affect the position of equilibrium for this reaction.
Question 18
5 marks · Hard
Answer and see the solution →The equation for a reaction that reaches equilibrium in a sealed container is:
A student investigates how changing the pressure affects this equilibrium.
(a)[1 mark]State the total number of moles of gaseous molecules on each side of the equation.
(b)[2 marks]Predict, with a reason, what will happen to the position of equilibrium if the pressure in the container is increased.
(c)[2 marks]If the pressure is decreased, which side of the equilibrium will be favoured? Explain your answer.
Question 19
2 marks · Hard
Answer and see the solution →Explain, using the idea of gaseous molecules, why changing the pressure does not influence the equilibrium position in reactions involving only solids and liquids.