Equilibria

Quiz by Horia

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28 questions
• Q1

What is a reversible reaction?

A reaction in which products can make reactants and the products can re make the reactants.

A reaction in which reactants can make products and the products can re make the reactants.

30s
• Q2

Considering the reaction: nitrogen + hydrogen ⇌ ammonia  - what is the backward reaction?

ammonia --> nitrogen + hydrogen

ammonia --> nitrogen + hydrogen

nitrogen + hydrogen --> ammonia

30s
• Q3

Considering the reaction: nitrogen + hydrogen ⇌ ammonia  - what is the forward reaction?

ammonia --> nitrogen + hydrogen

nitrogen + hydrogen --> ammonia

30s
• Q4

What is meant by ‘dynamic equilibrium’?

A reversible reaction occurring in a closed system with the forward and backward reactions occurring at the same constant. The concentrations of the reactants and the products remain rate

A reversible reaction occurring in a closed system with the forward and backward reactions occurring at the same rate. The concentrations of the reactants and the products remain constant

30s
• Q5

What does Le Chatelier’s principle state?

If any factor is changed which affects the equilibrium mixture, the position of the equilibrium will shift to oppose the change.

If any factor is changed which affects the equilibrium mixture, the position of the equilibrium will shift to exaggerate the change.

30s
• Q6

If the backward reaction is favoured in an equilibrium mixture, which direction does the equilibrium position shift to?

The equilibrium position shifts to the right – increasing the yield of the products.

The equilibrium position shifts to the right – increasing the yield of the products.

The equilibrium position shifts to the left – increasing the yield of the reactants.

30s
• Q7

If the forward reaction is favoured in an equilibrium mixture, which direction does the equilibrium position shift to?

The equilibrium position shifts to the left – increasing the yield of the reactants.

The equilibrium position shifts to the right – increasing the yield of the products.

30s
• Q8

A + B ⇌ C + D

If the concentration of C is increased– what happens to the equilibrium position?

The backward reaction is favoured – the equilibrium position shifts to the left. This lowers the concentration of C.

The forward reaction is favoured – the equilibrium position shifts to the left. This lowers the concentration of C.

The forward reaction is favoured – the equilibrium position shifts to the left. This lowers the concentration of A.

The forward reaction is favoured – the equilibrium position shifts to the right. This lowers the concentration of A.

30s
• Q9

A + B ⇌ C + D

If the concentration of A is increased– what happens to the equilibrium position?

The backward reaction is favoured – the equilibrium position shifts to the left. This lowers the concentration of C.

The forward reaction is favoured – the equilibrium position shifts to the left. This lowers the concentration of C.

The forward reaction is favoured – the equilibrium position shifts to the left. This lowers the concentration of A.

The forward reaction is favoured – the equilibrium position shifts to the right. This lowers the concentration of A.

30s
• Q10

A + B ⇌ C + D

If the concentration of B is decreased – what happens to the equilibrium position

The forward reaction is favoured – the equilibrium position shifts to the left. This increases the concentration of B.

The backward reaction is favoured – the equilibrium position shifts to the right. This increases the concentration of B.

The backward reaction is favoured – the equilibrium position shifts to the left. This increases the concentration of B.

30s
• Q11

A + B ⇌ C + D         ΔH° = - 50kJ/mol

What does this tell you about the reaction?

backward reaction is exothermic

backward reaction is endothermic

forward reaction is exothermic

forward reaction is endothermic

30s
• Q12

A + B ⇌ C + D        ΔH° = - 50kJ/mol. The temperature is decreased – what happens?

The forward reaction is favoured – the equilibrium position shifts to the right. This increases the temperature again.

The backward reaction is favoured – the equilibrium position shifts to the left. This reduces the temperature again.

The forward reaction is favoured – the equilibrium position shifts to the right. This reduces the temperature again.

The backward reaction is favoured – the equilibrium position shifts to the left. This increases the temperature again.

30s
• Q13

A + B ⇌ C + D        ΔH° = - 50kJ/mol. The temperature is increased – what happens?

The backward reaction is favoured – the equilibrium position shifts to the left. This reduces the temperature again.

The forward reaction is favoured – the equilibrium position shifts to the right. This increases the temperature again.

The backward reaction is favoured – the equilibrium position shifts to the left. This increases the temperature again.

The forward reaction is favoured – the equilibrium position shifts to the right. This reduces the temperature again.

30s
• Q14

2A + B ⇌ C + D The pressure is increased – what happens?

The forward reaction is favoured; the equilibrium position shifts to the right as there are fewer moles of gas on the right-hand side. This increases the pressure.

The forward reaction is favoured; the equilibrium position shifts to the right as there are fewer moles of gas on the right-hand side. This decreases the pressure.

The backward reaction is favoured; the equilibrium position shifts to the left as there are more moles of gas on the left-hand side. This increases the pressure.

The backward reaction is favoured; the equilibrium position shifts to the left as there are more moles of gas on the left-hand side. This decreases the pressure.

30s
• Q15

2A + B ⇌ C + D The pressure is reduced – what happens?

The backward reaction is favoured; the equilibrium position shifts to the left as there are more moles of gas on the left-hand side. This decreases the pressure.

The forward reaction is favoured; the equilibrium position shifts to the right as there are fewer moles of gas on the right-hand side. This decreases the pressure.

The backward reaction is favoured; the equilibrium position shifts to the left as there are more moles of gas on the left-hand side. This increases the pressure.

The forward reaction is favoured; the equilibrium position shifts to the right as there are fewer moles of gas on the right-hand side. This increases the pressure.

30s

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