A mixture of gases which are rich in hydrocarbons, consisting largely of methane.

Refers to the raw materials used in chemical processes to produce other substances.

The starting materials used to make products are known as the raw materials.

An industrial method for producing ammonia from nitrogen and hydrogen.

Industrial equilibria: Haber Process

Chemistry

Transition metals: properties and uses

Corrosion and its prevention: including half equations

Introduction to reversible chemical reactions

Chemical equilibrium

Industrial equilibria: Contact Process

Factors affecting equilibrium

Percentage yield and atom economy (RAM 1 d.p.)

Equilibrium: balance between rate, safety, environment and economics

Making ammonia

Ammonia: NPK fertiliser production and other applications

Comparing materials and their properties

In the Rates and energy changes unit, pupils learned about how energy changes are always involved in reaction, along with a range of methods for measuring and comparing rates of reaction using properties of reactants and/or products.

This unit covers corrosion, prevention methods, and properties of alloys, ceramics, polymers, and metals. It explores industrial processes like the Haber process, fertiliser production, reaction rates, yields, atom economy, and the trade-offs involving conditions and equilibrium.

Industrial chemistry

traditional ammonia, but involving carbon capture of the emissions

ammonia produced through 100% renewable and carbon-free processes

Traditional ammonia produced through the Haber process is called grey ammonia. Match the following terms with the correct definitions.

ammonia production is a reversible reaction

at equilibrium, there is ammonia but also nitrogen and hydrogen

high pressures require strong equipment and a lot of energy

high temperature is needed to increase the rate of reaction

nitrogen and hydrogen are wasted when ammonia is condensed and removed

Grey ammonia, through the Haber process, is the most common. Industrial production requires high pressure, large but safe apparatus, and a lot of energy. Which of the following statements are correct?

The conditions for the Haber process are:

nitrogen (from air) and hydrogen (from natural gas) are brought together

a compressor increases the pressure to 200 atm

the gas mixture is heated to 450$$^o$$C in a tank containing iron catalyst

the mixture enters a cooling tank so that ammonia is condensed

unreacted nitrogen and hydrogen are recycled to make more ammonia

In industry, ammonia is made with nitrogen from air, and hydrogen from natural gas, using the Haber process. Put the steps in order:

she felt passionately that science must not be used for chemical warfare

she thought making ammonia was a bad influence on people’s health

she was forced to stop being a chemist because he was already a chemist

Clara, Haber’s wife, was a chemist and pacifist, believing war and violence are unjustifiable. She felt her husband’s research was a “perversion of the ideals of science”. What made her feel that way?

As the global population continues to grow, production of ammonia will continue. What is ammonia **not** used for?

equal reaction rates for forward and backward reaction

Which of these statements are required for a dynamic equilibrium to be established?

The direction of reversible reactions can be influenced by changing conditions, e.g. an exothermic reaction is favoured by lowering the temperature, but at the same time the reaction rate {{}}.

True or false? At dynamic equilibrium all bonds between all atoms need to be broken and new bonds need to be formed.

the carbon dioxide gas leaves and the backward reaction can no longer occur

the forward reaction stops and you are left with only calcium carbonate

there will be an equilibrium with only calcium carbonate and calcium oxide

Consider this reaction:
CaCO$$_3(s)$$ ⇌ CaO$$_(s)$$ + CO$$_2(g)$$
What would happen if this was done in an open system?

Industrial chemistry is different from chemistry in a school lab or a research lab. The {{}} of the work is larger; therefore the risks and safety measures are larger too.

at equilibrium the rates of the forward and backward reaction must be equal

the graphs for the forward and backward reaction have been swapped

the reactants and products should be mentioned in a rate of reaction graph

Industrial equilibria: Haber Process

Lesson outcome