Equilibrium Topic 7 Unit 2

Question 1

What is a irreversible reaction

Answer 1

A reaction where reactants cannot change into products but the products cannot change back into the reactants

Question 2

What are examples of irreversible reactions

Answer 2

Baking a cake, burning a newspaper and magnesium with acid

Question 3

What is a reversible reaction

Answer 3

A reaction where reactants can change into products and the products can change back into the reactants

Question 4

What is an equilibrium?

Answer 4

Reversible reactions that happen in a closed system eventually reach an equilibrium

Question 5

What is an open system?

Answer 5

If a chemical reaction happens in a container where one or more of the reactants or products can escape.

Question 6

What is a closed system?

Answer 6

When a chemical reaction happens in a container where none of the products or reactants can escape.

Question 7

What is dynamic equilibrium?

Answer 7

When the rate of forward reaction is equal to the rate of reverse reaction resulting in the amount of reactants and products remaining constant

Question 8

What happens if there are more products than reactants?

Answer 8

The position of equilibrium is to the right-hand side

Question 9

What happens if there are more reactants than products?

Answer 9

Position of equilibrium is to the left

Question 10

What is the position of equilibrium in a reversible reaction?

Answer 10

A measure of how far the reaction has went to the right (towards products) or has it stayed at the left (towards reactants)

Question 11

What is le châtelier’s principle?

Answer 11

If a change is made to the conditions of a system at equilibrium, then the position of equilibrium moves to oppose the change in conditions.

Question 12

What is a homogenuous reaction?

Answer 12

All the reactants and products are in the same state.

Question 13

What is the change of concentration in the lungs?

Answer 13

The concentration of oxygen increases and then there is a shift of the equilibrium to the right.

Question 14

What is the change in concentration in the tissues?

Answer 14

The concentration of oxygen decreases and then the equilibrium shifts to lift.

Question 15

When does the equilbrium change under pressure?

Answer 15

If there is at least 1 gas present

Question 16

What happens if the pressure is increased?

Answer 16

The equilibrium will go to the right, creating more product

Question 17

What happens to the equilibrium if pressure is reduced?

Answer 17

The equilibrium will reduce to the left, resulting in more reactants

Question 18

What happens if the forward reaction is exothermic and temperature increased?

Answer 18

The yield of products is decreased

Question 19

What happens if the forward reaction is endothermic and temperature is increased?

Answer 19

The yield of products is increased

Question 20

What happens if temperature is increased?

Answer 20

Shift in endothermic direction

Question 21

What happens if the temperature is decreased?

Answer 21

Shift in exothermic direction

Question 22

What is the haber process?

Answer 22

The industrial manufacture of ammonia

Question 23

What happens to ammonia production at lower temperatures?

Answer 23

The yield of ammonia is better at lower temperature.

Question 24

What temperature is the haber process done at?

Answer 24

450°C - a high enough temperature for fast reaction and good amonia yield

Question 25

What happens to ammonia production if pressure is increased?

Answer 25

Position of equilibrium will go to the right and more ammonia is made

Question 26

Why is there a limit to pressur when making ammonia?

Answer 26

It’s dangerous - very high pressures = strong, expensive equipment

Question 27

What pressure is used for ammonia production?

Answer 27

200 atmospheres, high enough for a good yield but not so high for the costs.

Question 28

What catalyst is used for haber process?

Answer 28

Iron

Question 29

What does a catalyst do to equilibrium?

Answer 29

Nothing! Just speeds up rate of reaction