Propane burns in air according to the following equation :

C₃H₈ + 5O₂ ⟶ 3CO₂ + 4H₂O.

What volume of propane is consumed on using 1000 cm³ of air, considering only 20% of air contains oxygen.

Ethane burns in O₂ to form CO₂ and H₂O

2C₂H₆ + 7O₂ ⟶ 4CO₂ + 6H₂O

If 1250 cc. of oxygen is burnt with 300 cc of ethane.

Calculate :

(i) volume of CO₂ formed.

(ii) volume of unused O₂.

The volumes of gases A, B, C and D are in the ratio, 1 : 2 : 2 : 4 under the same conditions of temp. and press.

(i) Which sample contains the maximum no. of molecules. If the temp, and pressure of gas A are kept constant, what will happen to the volume of A when the no. of molecules is doubled.

(ii) If the volume of 'A' is 5.6 dm³ at s.t.p., calculate the no. of molecules in the actual vol. of 'D' at s.t.p. [Avog no. is 6 × 10²³).

Using your answer, state the mass of 'D' if the gas is N₂O

[N = 14, O = 16]

Calculate the no. of moles and the no. of molecules present in 1.4 g of ethylene gas (C₂H₄). What is the vol. occupied by the same amount of C₂H₄. State the vapour density of C₂H₄.

(Avog. No. = 6 × 10²³ ; C = 12, H = 1]