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Equilibria is a state of balance.

Equilibria

Equilibria is about reversible reactions reaching balance in a closed system. This GCSE Chemistry quiz helps you predict how changing conditions affects the equilibrium position.

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Fascinating Fact:

Dynamic equilibrium means particles are still reacting in both directions. There is no overall change because the rates are equal.

In GCSE Chemistry, equilibrium describes what happens in reversible reactions when the forward and reverse reactions occur at the same rate. You explore how concentration, pressure, and temperature can shift the equilibrium position and change the amounts of reactants and products.

Key Terms

Reversible Reaction: A reaction where products can react to form reactants, shown with a double arrow.
Equilibrium Position: The balance point showing the relative amounts of reactants and products at equilibrium.
Le Chatelier’s Principle: If conditions change, the system shifts to reduce the effect of that change.

Frequently Asked Questions

What is dynamic equilibrium in GCSE Chemistry?

Dynamic equilibrium is when a reversible reaction in a closed system has equal forward and reverse reaction rates, so the concentrations stay constant even though particles still react.

How does changing concentration affect the position of equilibrium?

Increasing the concentration of a reactant shifts equilibrium towards products to use it up, while increasing product concentration shifts equilibrium towards reactants to reduce the change.

How does pressure affect equilibrium in gas reactions?

Increasing pressure shifts equilibrium towards the side with fewer moles of gas, while decreasing pressure shifts it towards the side with more moles of gas, if the gases are in a closed system.

Try These Related Quizzes

1 .

How do we represent a reversible reaction symbolically?

→

←

↓

⇌

This shows the two directions that the reaction will proceed in, both forwards and reverse. Sometimes the arrow is drawn with a larger arrow in one direction to show the predominant reaction direction

2 .

At equilibrium, if the rate of the forward reaction increases, the rate of the reverse reaction...

increases until it is going at the same rate as the forward reaction

decreases until both reactions are going at the same rate

carries on at a steady rate

increases to faster than the forward reaction

At equilibrium, the rate of the forward and reverse reaction are the same. To compensate for the increased rate of the forward reaction, the reverse reaction must also increase

3 .

The Haber process is a reversible reaction. If the reaction were at equilibrium, hydrogen and nitrogen would be being produced as quickly as ammonia gas was being broken down. How is the forward reaction rate increased?

By removing nitrogen and hydrogen from the reaction vessel

By removing ammonia from the reaction vessel

By increasing the amount of hydrogen and nitrogen in the reaction vessel

By increasing the pressure

The system attempts to achieve equilibrium by increasing the rate of the forward reaction, i.e. by making more ammonia to replace that which has been removed

4 .

If a reversible reaction is exothermic in the forward direction, in the reverse direction it will be...

endothermic

exothermic

unknown - you cannot tell

slower

Knowing which direction of the reversible reaction is exothermic can help you to predict what might happen when the temperature is changed

5 .

A stable equilibrium can be achieved in a...

chemical system

open system

closed system

reaction system

A closed system is one in which no reactants or products can enter or leave

6 .

At the point of equilibrium...

the rate of the forward reaction is greater than the rate of the reverse reaction

the rate of the forward reaction is slower than the rate of the reverse reaction

the rate of the forward reaction is double the rate of the reverse reaction

the rate of the forward reaction is the same as the rate of the reverse reaction

At this point there is no overall change in the amount of products or reactants

7 .

What is a reversible reaction?

A reaction which will proceed in the forwards direction only

A reaction which will proceed in both forwards and backwards directions

A reaction which will proceed in the backwards direction only

A reaction which will not proceed in any direction

A good example of a reversible reaction is the formation of ammonia from hydrogen and nitrogen

8 .

At equilibrium, the amount of product(s) and reactant(s) is constant. Which of the following would increase the amount of product in a reaction?

Remove the product from the reaction vessel

Add more product to the reaction vessel

Increase the temperature of the reaction mixture

Increase the pressure of the reaction vessel

If the product is removed, there will be less of the reverse reaction occurring. The forward reaction will continue, forming more of the product to replace the quantity removed to re-establish the equilibrium. Adding more of the reactants would have the same effect

9 .

One example of a reversible reaction is the Haber process. Pick the correct symbol equation for the reaction between hydrogen and nitrogen to produce ammonia in the Haber process.

N₂ + 3H₂ → 2NH₃

N₂ + 3H₂ ← 2NH₃

N₂ + 3H₂ ⇌ 2NH₃

N₂ + 3H₂ ⇌ NH₃

You should have immediately dismissed the first two answers since they don't contain the double arrow that shows this is a reversible reaction. Ammonia is an important chemical in industry and is used to manufacture nitric acid and fertilisers

10 .

What effect will adding a catalyst have to the equilibrium of a system?

No effect, it just speeds up getting to the point of equilibrium

It will increase the rate of the forward reaction only

It will increase the rate of the reverse reaction only

It decreases the amount of product produced

It speeds up both the forward and reverse reactions equally

You can find more about this topic by visiting BBC Bitesize - Reversible reactions

Author: Kate Gardiner (Chemistry Educator & GCSE Quiz Writer)

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