Stoichiometry refers to the molar ratio of the reactants and products in a chemical reaction.

The relative formula mass of a substance is the sum of the relative atomic masses of all the atoms in a formula.

A mole of something is 6.02 × 10²³ of it. The mass of a mole of a substance is its relative mass expressed in grams.

Mass in a chemical reaction: using moles (RAM 1 d.p.)

Chemistry

In the Making salts unit, pupils will learn about the production of pure salts, concentration and strength of acids, and what makes acids acidic and how bases can neutralise them.

In the Atomic structure and periodic table unit, pupils learned about atoms, and how the periodic table is ordered, along with the history of both of their major discoveries.

Calculations involving masses

Measuring elements and their ratios in reactions.

The temperature changes in chemical reactions.

What does stoichiometry mean in chemistry?

The physical states of the reactants and products.

How many particles are involved in the reaction.

The proportions of substances that react or are produced.

In a balanced chemical equation, what does the mole ratio of reactants and products tell us?

The {{}} is the sum of the relative atomic masses of all the atoms in a formula, representing the mass of a molecule relative to the mass of a carbon-12 atom.

Two molecules of hydrogen react with one molecule of oxygen.

Two moles of hydrogen are needed to react with one mole of oxygen.

Four hydrogen atoms react with two oxygen atoms.

Two hydrogens reacts with oxygen to make two lots of water.

Which of the following statements best describes what the equation 2H₂ + O₂ → 2H₂O tells us?

Given the reaction: CH₄ + 2O₂ → CO₂ + 2H₂O, how many grams of CO₂ are produced when 16 g of methane (CH₄) reacts completely? Relative formula mass values: (CH₄ = 16.0) and (CO₂ = 44.0)

Using the reaction: N₂ + 3H₂ → 2NH₃, calculate the mass of ammonia (NH₃) produced when 14 g of nitrogen react with hydrogen? (2 s.f.)
Relative formula mass values: (N₂ = 28.0) & (NH₃ = 17.0)

Given the relative atomic masses (Ar): C (12.0), O (16.0).
Calculate the relative formula mass (Mr) of carbon dioxide (CO₂).

Mass of products is always more than the mass of reactants.

Mass of reactants is converted into energy.

Mass of reactants equals mass of products.

What does the conservation of mass in a chemical reaction imply?

If 20 g of sodium reacts fully with 15 g of chlorine, how much sodium chloride is produced?

For the equation __ N₂ + __ H₂ → __ NH₃, select the correct coefficients to balance it.

Two molecules of hydrogen react with two molecules of oxygen.

One molecule of hydrogen reacts with one molecule of oxygen.

Two molecules of water are decomposed into hydrogen and oxygen.

What does the equation 2H₂ + O₂ → 2H₂O tell us?

Given the relative atomic mass values (Ar): H (1.0), S (32.1), O (16.0).
Calculate the relative formula mass (Mr) of sulfuric acid.

This lesson will soon be taken down.

Mass in a chemical reaction: using moles (RAM 1 d.p.)

Lesson outcome