Have you heard of Le Chatelier’s Principle?
Dynamic Equilibrium Quiz
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Question 1 of 13Question 1
Some chemical reactions are reversible. What does this mean?
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Question 2 of 13Question 2
Which of the following symbols is used to represent a reversible reaction?
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Question 3 of 13Question 3
Use the following words to fill in the blanks:
Open, closed, active, dynamic, static
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- equilibrium only occurs in systems.
- In an system gases can escape so equilibrium would not be achieved.
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Question 4 of 13Question 4
Which of the following explains dynamic equilibrium?
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Question 5 of 13Question 5
Which of the following are conditions that are used during the Haber process?
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Question 6 of 13Question 6
Ammonia is produced during which process?
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Question 7 of 13Question 7
Ammonia is produced as a reversible reaction between which elements?
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Question 8 of 13Question 8
Use some of the following words to fill in the blanks:
Hydrogen, nitrogen, oxygen, chlorine, air, natural, artificial, water
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Complete the statements about the elements used in the process to make ammonia:
- is extracted from the .
- is obtained from gas
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Question 9 of 13Question 9
Can the process used to obtain ammonia achieve dynamic equilibrium?
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Question 10 of 13Question 10
The environment in which a reaction takes place can affect the direction of the equilibrium shift.
A reaction is exothermic in the forwards direction. Match the change in temperature with the correct outcome.
- Equilibrium shifts to the left
- Equilibrium shifts to the right
- Increasing temperature
- Decreasing temperature
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Question 11 of 13Question 11
The environment in which a reaction takes place can affect the direction of the equilibrium shift.
Hydrogen reacts with iodine to form hydrogen iodide. Match the change with the correct outcome.
H₂(g) + I₂(g) ⇌ 2HI(g)- Equilibrium shifts to the right
- Equilibrium shifts to the left
- H₂ is added
- H₂ is removed
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Question 12 of 13Question 12
The environment in which a reaction takes place can affect the direction of the equilibrium shift.
Hydrogen reacts with iodine to form hydrogen iodide. Match the change with the correct outcome.
H₂(g) + I₂(g) ⇌ 2HI(g)Fill in the blanks with the following terms:
Right, left
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Match the following changes with the correct outcome:
- Increasing the concentration of H₂ will shift the equilibrium to the .
- Decreasing the pressure of I₂ will shift the equilibrium to the .
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Question 13 of 13Question 13
There is a dynamic equilibrium formed in the following reaction: nitrogen dioxide ⇌ dinitrogen tetroxide. Which of the following will happen if we add more nitrogen dioxide?
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