HI = Chemical equilibrium / Haber process

Question 1

Define dynamic equilibrium

Answer 1

The rate of the forward and backward reactions are equal

Question 2

1-Equation for the Haber process

2-What type of reaction if the forward reaction? (Delta H)

3-What happens when you increase the pressure?

4-What happens when you increase the temperature?

Answer 2

1 - 3H2(g) + N2(g) 2NH3(g)

2 - Exothermic

3 - Moles of reactants : products is 4:2 so an increased pressure will favour products

4-Favours reactants as the forward reaction is exothermic

Question 3

Describe an experiment that show cases a reversible reaction

Answer 3

HYDRATED COPPER (II) SULPHATE SOLID

1-Place one spatula of copper(II) sulphate powder into a boiling tube

2-Heat the boiling tube over a bunsen burner (blue flame)

3-Copper(II) sulphate is white when it is anhydrous (after heating it).
It will turn blue again if you add water to it

Question 4

Conditions for Haber process (3)

Answer 4

• Low temperature = 450 degrees C
• High pressure = 200 atm
• Iron (III) catalyst

Question 5

1 - Raw materials of the Haber process (2)

2 - How do you obtain the raw materials?

Answer 5

1-Nitrogen and hydrogen

2-Nitrogen comes from the air and hydrogen is usually obtained through either cracking or reacting natural gases e.g. methane with steam

Question 6

Uses of Ammonia (3)

Answer 6

• Making medicines
• Making fertilizers
• Making explosives

Question 7

What if the purpose of the Haber process?

Answer 7

To produce ammonia

Question 8

General formula for an equilibrium reaction?

Answer 8

A + B C + D

Question 9

Chemical equilibrium law?

Answer 9

Le Chantelier’s principle

When a reversible reaction is in equilibrium and you make a change, the system acts to oppose the change, and restore equilibrium. A new equilibrium mixture forms