A chemist reacts sulfur completely with chlorine to make an unknown molecular compound. The masses of the elements that combine are shown in the table.
| Element | Mass that combines |
|---|---|
| Sulfur | 3.20 g |
| Chlorine | 3.55 g |
The relative atomic masses are S = 32 and Cl = 35.5. The relative formula mass (MrM_rMr) of the compound is 135.
Calculate the empirical formula of the compound.
Calculate the molecular formula of the compound.
142 exam-style questions on Edexcel GCSE Chemistry 2.6 Calculations involving masses, covering 2.6.1 Relative formula mass and percentage composition, 2.6.2 Empirical and molecular formulae, 2.6.3 Conservation of mass, 2.6.4 Reacting masses and concentration in g dm⁻³, 2.6.5 The mole and the Avogadro constant, and 2.6.6 Limiting reactants and stoichiometry. Each one has a worked solution and a mark scheme showing where the marks go.