Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Physical Chemistry
442 practice questions
Topics covered
Practice questions
141–150 of 188 · Normal
Question 141
2 marks · Normal
Answer and see the solution →A reversible reaction occurs in a sealed container: . The forward reaction is exothermic.
State what happens to the position of equilibrium if:
(a)[1 mark]the temperature is increased.
(b)[1 mark]the pressure is increased.
Question 142
4 marks · Normal
Answer and see the solution →Consider the following equilibrium established in a sealed container:
The forward reaction is endothermic.
(a)[2 marks]State and explain what will happen to the position of equilibrium if the temperature is decreased.
(b)[2 marks]State and explain what will happen to the position of equilibrium if the pressure is increased.
Question 143
3 marks · Normal
Answer and see the solution →The following equilibrium is established in a sealed container at constant temperature:
The forward reaction is exothermic.
The system is at equilibrium with the following amounts:
Substance Amount (mol) D 0.80 E 1.60 F 0.60 G 0.60 (a)[3 marks]The pressure on the system is increased. Predict, with a calculation, which direction the equilibrium will shift. Show your working.
Question 144
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 145
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 146
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 147
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 148
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 149
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 150
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.