is the maximum calculated mass of product expected to form from a given mass of reactants

is the actual amount of product obtained from a chemical reaction

is the actual yield (mass of product obtained) divided by the theoretical yield (maximum mass of product possible), as a percentage

is the percentage, by relative mass, of reactants that are converted into useful products

is a chemical product that is desired or valuable

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

Chemistry

Transition metals: properties and uses

Corrosion and its prevention: including half equations

Introduction to reversible chemical reactions

Chemical equilibrium

Industrial equilibria: Haber Process

Industrial equilibria: Contact Process

Factors affecting equilibrium

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

Maximum calculated mass of product expected to form in a reaction.

Amount of product obtained from a chemical reaction.

Percentage of reactants converted into useful products.

Match the following terms to the correct definitions.

During an experiment, a pupil produces 3.25 g of magnesium oxide. The theoretical yield of magnesium oxide is 4.00 g.
Calculate the percentage yield. Give your answer to 3 s.f.

All the reactants are used in the reaction.

Why might the percentage yield of a reaction not be 100%?

Calculate the theoretical yield of magnesium oxide when 2.40 g of magnesium reacts with excess oxygen. Give your answer to 3 s.f.
2Mg + O₂ → 2MgO.
Relative atomic masses (Ar): Mg = 24.3; O = 16.0.

It is a measure of the efficiency of how a reaction uses its reactants.

It shows how actual yield compares to theoretical yield.

Which of the following statements about atom economy are correct?

Calculate the percentage atom economy of the reaction below, when hydrogen is the useful product. Give your answer to 3 s.f.
2H₂O → O₂ + 2H₂.
Relative atomic masses (Ar): H = 1.0; O = 16.0.

Three beads are red and seven beads are green. What percentage of the beads are green?

Balance the following chemical equation:
CH₄ + O₂ → H₂O + CO₂ 

Calculate the relative formula mass (Mr) of calcium carbonate, CaCO₃. 
Relative atomic masses (Ar): Ca = 40.1; C = 12.0; O = 16.0.

The ratio of magnesium atoms to magnesium oxide is 1 : 1.

The ratio of magnesium oxide to oxygen atoms is 1 : 2.

The ratio of oxygen atoms to magnesium atoms is 1 : 2.

The ratio of oxygen atoms to magnesium oxide is 2 : 1.

Which of the following statements about the equation below are correct?
2Mg + O₂ → 2MgO

When magnesium reacts with oxygen in the air to form magnesium oxide, magnesium is the limiting factor. There is more oxygen present than is needed, so we say that the oxygen is in {{}}.

Calculate the mass of 0.50 mol of magnesium. Give your answer to 3 s.f.
Relative atomic mass (Ar) of Mg = 24.3. 

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

Lesson outcome