10 mL of liquid carbon disulphide (specific gravity 2.63) is burnt in oxygen. Find the volume of the resulting gases measured at STP.

CS₂ + 3O₂ →  CO₂ + 2SO₂
Volume of CS₂ = 10ml
density of CS₂ = 2.63g/ml
Weight of CS₂ = 2.63(10) = 26.3g
CS₂ + 3O₂ →  CO₂ + 2SO₂
  76g               22.4l    (2 x 224l)
   26.3g            'X₁l'        'X₂'l
$$\begin{gathered} {\mathrm{X}}_1 =\frac{26.3}{76}\times 22.4 =7.75 \mathrm{l} \\ {\mathrm{X}}_2 =\frac{26.3}{76}\times 2\times 22.4 =15.5\mathrm{l} \end{gathered}$$

Total volume of gases liberated STP  = (15.5 + 7.75) lit
                                                     = 23.25 lit