Ethane, C2H6\text{C}_2\text{H}_6C2H6, burns completely in oxygen to produce carbon dioxide and water vapor according to the following equation:
2C2H6+7O2→4CO2+6H2O 2\text{C}_2\text{H}_6 + 7\text{O}_2 \rightarrow 4\text{CO}_2 + 6\text{H}_2\text{O} 2C2H6+7O2→4CO2+6H2OCalculate the minimum volume of air, measured at room temperature and pressure, required to burn 60 g of ethane completely.
Assume that air contains 21% oxygen by volume.
(Relative atomic masses, ArA_rAr: C=12\text{C} = 12C=12, H=1\text{H} = 1H=1; 1 mol of gas occupies 24 dm3 at room temperature and pressure)
157 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.