(a) (i) A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correct to 1 decimal place. (H = 1; C = 12; Cl = 35.5)(ii) The relative molecular mass of this compound is 168, so what is its molecular formula?(iii) By what type of reaction could this compound be obtained from ethyne?(b) From the equation:C + 2H2SO4 → CO2 + 2H2O + 2SO2Calculate:(i) the mass of carbon oxidised by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98).(ii) the volume of sulphur dioxide measured at STP, liberated at the same time.(Volume occupied by 1 mole of a gas at STP is 22.4 dm3).

(a) (i) A compound has the following percentage composition by mass: c

1.	(a) (i) A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correct to 1 decimal place. (H = 1; C = 12; Cl = 35.5)(ii) The relative molecular mass of this compound is 168, so what is its molecular formula?(iii) By what type of reaction could this compound be obtained from ethyne?(b) From the equation:C + 2H2SO4 → CO2 + 2H2O + 2SO2Calculate:(i) the mass of carbon oxidised by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98).(ii) the volume of sulphur dioxide measured at STP, liberated at the same time.(Volume occupied by 1 mole of a gas at STP is 22.4 dm3).
Answer» (a) (i) A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correct to 1 decimal place. (H = 1; C = 12; Cl = 35.5) (ii) The relative molecular mass of this compound is 168, so what is its molecular formula? (iii) By what type of reaction could this compound be obtained from ethyne? (b) From the equation: C + 2H₂SO₄ $\overset{}{\to}$ CO₂ + 2H₂O + 2SO₂ Calculate: (i) the mass of carbon oxidised by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98). (ii) the volume of sulphur dioxide measured at STP, liberated at the same time. (Volume occupied by 1 mole of a gas at STP is 22.4 dm³).