From the equation.:

C + 2H₂SO₄ → CO₂ + 2H₂O +2SO₂

Calculate:

The volume of sulphur dioxide measured at STP, liberated at the same time.

(Volume occupied by 1 mole of a gas at STP is 224 dm³)

Q.

(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 $\stackrel{}{\to }$ 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).

Q. The volume occupied by half a mole of a gas at STP is:

Q. The volume occupied by 1 mole atom of a diatomic gas at STP is:

Q. Calculate the volume of $S{O}_2$ SO2_ produced for 49g of $H_{2}S{O}_4$ at STP.

Q. (a) What is the volume occupied by the following gases at STP?
(i) 48 g of oxygen.
(ii) 16 g of sulphur dioxide
(b) Determine the molecular mass of a gas if 5 g of it occupies a volume of 4 litres at STP.