720 dm3 of dinitrogen tetroxide, measured at room temperature and pressure, decomposed to form nitrogen dioxide.
N2O4(g)⇌2NO2(g) \text{N}_2\text{O}_4(\text{g}) \rightleftharpoons 2\text{NO}_2(\text{g}) N2O4(g)⇌2NO2(g)Calculate the maximum mass, in kg, of nitrogen dioxide formed in this reaction. (Relative atomic masses: N=14.0\text{N} = 14.0N=14.0, O=16.0\text{O} = 16.0O=16.0; 1 mol of any gas at room temperature and pressure occupies 24 dm3)
119 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.