(a) What volume of oxygen is required to burn completely a mixture of 22.4 dm3 of methane and 11.2 dm3 of hydrogen into carbon dioxide and steam? Equations of the reactions are given below:CH4 + 2O2 → CO2 + 2H2O2H2 + O2 → 2H2O(Assume that all volumes are measured at STP)(b) The gases hydrogen, oxygen, carbon dioxide, sulphur dioxide and chlorine are arranged in order of their increasing relative molecular mass. Given 8 g of each gas at STP, which gas will contain the least number of molecules and which gas the most?

(a) What volume of oxygen is required to burn completely a mixture of

1.	(a) What volume of oxygen is required to burn completely a mixture of 22.4 dm3 of methane and 11.2 dm3 of hydrogen into carbon dioxide and steam? Equations of the reactions are given below:CH4 + 2O2 → CO2 + 2H2O2H2 + O2 → 2H2O(Assume that all volumes are measured at STP)(b) The gases hydrogen, oxygen, carbon dioxide, sulphur dioxide and chlorine are arranged in order of their increasing relative molecular mass. Given 8 g of each gas at STP, which gas will contain the least number of molecules and which gas the most?
Answer» (a) What volume of oxygen is required to burn completely a mixture of 22.4 dm³of methane and 11.2 dm³ of hydrogen into carbon dioxide and steam? Equations of the reactions are given below: CH₄ + 2O₂ $\overset{}{\to}$ CO₂ + 2H₂O 2H₂ + O₂ $\overset{}{\to}$ 2H₂O (Assume that all volumes are measured at STP) (b) The gases hydrogen, oxygen, carbon dioxide, sulphur dioxide and chlorine are arranged in order of their increasing relative molecular mass. Given 8 g of each gas at STP, which gas will contain the least number of molecules and which gas the most?