Reversible Reactions (Dynamic Equilibrium + Haber Process)

Question 1

What is meant by a reversible reaction?

Answer 1

A reaction that can occur in either direction

Question 2

What is the symbol for a reversible reaction?

Answer 2

⇌

Question 3

What is meant by the term dynamic equilibrium?

Answer 3

Rate of forward and reverse reactions occur at the same rate

Question 4

What needs to happen for equilibrium to be reached?

Answer 4

Needs to be in a closed system; products and reactants cannot escape

Question 5

The formation of ammonia is a reversible reaction between what?

Answer 5

Nitrogen and hydrogen

Question 6

Where are the reactants for the formation of ammonia extracted from?

Answer 6

Hydrogen - natural gas

Nitrogen - air

Question 7

Name three conditions for the Haber process

Answer 7

Temperature - 450˚C
Pressure - 200 atmospheres
Iron catalyst

Question 8

What is the equation for the production of ammonia?

Answer 8

3H2 + N2 ⇌ 2NH3

Question 9

What three factors can be changed in a system at equilibrium?

Answer 9

Concentration, temperature and pressure

Question 10

If the concentration of a reactant is increased, what will happen to the products of the reaction?

Answer 10

More products will be produced until equilibrium is reached

Question 11

What will happen to the amount of product in an endothermic reaction at equilibrium if the temperature is increased?

Answer 11

More products will be produced

Question 12

What will happen to the amount of product in an exothermic reaction at equilibrium if the temperature is increased?

Answer 12

Relative amount of products will decrease

Question 13

What will happen to the amount of product in an endothermic reaction at equilibrium if the temperature is decreased?

Answer 13

Relative amount of products will decrease

Question 14

What is meant by the term: gaseous reaction?

Answer 14

Reaction where all the reactants and products are gases

Question 15

What would happen to the position of equilibrium in a gaseous reaction if the pressure is increased?

Answer 15

Equilibrium would shift towards the side with the smaller number of molecules shown in the balanced chemical equation

Question 16

Explain what will happen in the following reaction if we increase the concentration of the hydrogen and iodine:
I2(g) + H2(g) ⇌ 2HI (g)

Answer 16

The extra iodine and hydrogen will react together to make more hydrogen iodide

Question 17

What will happen if we increase the temperature of the reaction below? (Explain why)
N2(g) + 3H2(g) ⇌ 2NH3(g)

Answer 17

More hydrogen and nitrogen will be made as the backward reaction is endothermic

Question 18

Explain what will happen if we decrease the pressure in this reaction:
N2(g) + 3H2(g) ⇌ 2NH3(g)

Answer 18

We will get more nitrogen and hydrogen as there are four moles of gas/higher volume for the reactants