6.7 Reversible Reactions & Dynamic Equilibrium

Question 1

What is a reversible reaction?

Answer 1

A reversible reaction is one where the products can react with each other to produce the original reactants. In other words, it can go both ways.

Question 2

In what can equilibrium reactions only take place in?

Answer 2

A ‘closed system’.

Question 3

What does it mean when the equilibrium lies to the right?

Answer 3

The concentration of products is greater than the concentration of reactants

Question 4

What does it mean when the equilibrium lies to the left?

Answer 4

The concentration of reactants is greater than the concentration of products

Question 5

In a system that’s closed, why can the yield of a reversible reaction never be 100%?

Answer 5

There will always be a mixture of products and reactants, even if the equilibrium lies very far to the right or to the left.

Question 6

What are the three things that can change the position of equilibrium?

Answer 6

1) Temperature
2) Pressure
3) Concentration

Question 7

Does adding heat increase the forward or backward reaction of a reversible reaction?

Answer 7

Forward reaction

Question 8

Summary of reversible reactions

Answer 8

• Reversible reactions are those with a double arrow in the middle which shows that they can react in both a forward and a backward direction. One of which will have to be exothermic and one will be endothermic.
• If these two reactions are the same, we say the reaction is at equilibrium and the concentrations of the reactants and products will remain constant.
• The position of equilibrium can shift to the left or right depending on the conditions.

Question 9

Dynamic equilibrium (3)

Answer 9

• The concentrations of the reactants and products remain constant
• It requires a closed system
• The forward and backward reactions occur at the same rate