Equal moles of hydrogen and oxygen gases are placed in a container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the hydrogen to escape?

• 1/4

• 3/8

• 1/2

• 1/2

Liquid ‘M’ and liquid ‘N’ form an ideal solution. The vapour pressures of pure liquids ‘M’ and ‘N’ are 450 and 700mm Hg, respectively, at the same temperature. Then correct statement is:

(x_M = Mole fraction of 'M' is solution; x_N = Mole fraction of 'N' in solution; y_M = Mole fraction of 'M' in vapour phase; y_N = Mole fraction of 'N' in vapour phase)

• $\frac{{\mathrm{x}}_{\mathrm{M}}}{{\mathrm{x}}_{\mathrm{N}}} < \frac{{\mathrm{y}}_{\mathrm{M}}}{{\mathrm{y}}_{\mathrm{N}}}$

• $\frac{{\mathrm{x}}_{\mathrm{M}}}{{\mathrm{x}}_{\mathrm{N}}} = \frac{{\mathrm{y}}_{\mathrm{M}}}{{\mathrm{y}}_{\mathrm{N}}}$

• $\frac{{\mathrm{x}}_{\mathrm{M}}}{{\mathrm{x}}_{\mathrm{N}}} > \frac{{\mathrm{y}}_{\mathrm{M}}}{{\mathrm{y}}_{\mathrm{N}}}$

• (x_M - y_M) < (x_N - y_N)

1.0 g of magnesium is burnt with 0.56 g of O₂ in a closed vessel. Which reactant is left in excess and how much?

• Mg, 0.16 g

• O₂, 0.16 g

• Mg, 0.44 g

• Mg, 0.44 g

When 22.4 L of H₂ (g) is mixed with 11.2 L of Cl₂ (g), each of at STP, the moles of HCl (g) formed is equal to

• 1 mole of HCl (g)

• 2 moles of HCl (g)

• 0.5 mole of (g) 

• 0.5 mole of (g) 

Equal masses of H₂, O₂ and methane have been taken in a container of volume V at temperature 27⁰ C in identical conditions. The ratio of the volumes of gases H₂ : O₂: CH₄ would be 

• 8:16:1

• 16:8:1

• 16:1:2

• 16:1:2