Imagine baking a cake. You use exactly 200 g of flour, 150 g of sugar, and 100 g of butter. When you take the cake out of the oven it weighs roughly 450 g — the same as everything you put in. Nothing has been created. Nothing has been destroyed. Chemistry works exactly the same way. When iron rusts, when wood burns, when acids react with metals, the total mass of the atoms before and after is always identical. This single idea — conservation of mass — underpins every balanced equation you will ever write.
This introduction covers The Recipe That Never Wastes Anything within Formulae, Equations and Conservation of Mass for GCSE Chemistry. Revise Formulae, Equations and Conservation of Mass in Quantitative Chemistry for GCSE Chemistry with 13 exam-style questions and 12 flashcards. This topic shows up very often in GCSE exams, so students should be able to explain it clearly, not just recognise the term. It is section 1 of 14 in this topic. Use this introduction to connect the idea to the wider topic before moving on to questions and flashcards.
Practice questions for Formulae, Equations and Conservation of Mass
Which of the following is the correct formula for oxygen gas?
Explain why mass is conserved in a chemical reaction.
Quick recall flashcards
Name the seven diatomic elements.
H₂, N₂, O₂, F₂, Cl₂, Br₂, I₂
Mnemonic: Have No Fear Of Ice Cold Beer
State the law of conservation of mass.
In a chemical reaction, the total mass of the products equals the total mass of the reactants.
No atoms are created or destroyed — they are only rearranged.