Hydrogen reacts with chlorine according to the equation
H2(g)+Cl2(g)→2HCl(g)\mathrm{H_2(g) + Cl_2(g) \rightarrow 2HCl(g)}H2(g)+Cl2(g)→2HCl(g)
A mixture contains 80 cm3 of hydrogen and 55 cm3 of chlorine. The reaction continues until one reactant is completely used up. All gas volumes are measured at the same temperature and pressure.
Calculate the volume of hydrogen chloride formed and the volume of the excess reactant remaining.
151 exam-style questions on Edexcel GCSE Chemistry 6.2 Quantitative analysis, covering 6.2.1 Concentration in mol dm⁻³ and titration calculations, 6.2.2 Percentage yield and why actual yield falls short, 6.2.3 Atom economy of a reaction, 6.2.4 Choosing a reaction pathway, and 6.2.5 Molar volume of gases and Avogadro's law. Each one has a worked solution and a mark scheme showing where the marks go.