A gaseous mixture of `H_2 and CO_2` gases contains 66 mass % of `CO_2`. The vapour density of the mixture is :

A mixture contains N_(2)O_(4) and NO_(2) in the ratio 2:1 by volume. The vapour density of the mixture is:

A gascous mixture contains 56 g N_2, 44 g CO_(2) and 16 g CH_(4) . The total pressure of mixture is 720 mm. What is partial pressure of CH_(4) ?

Calculate the vapour pressure of an aqueous solution containing 5% by mass of urea (NH_2CON_2) at 298K. The vapour pressure of water at 298K is 23.75 mm Hg.

Two perfect gases at absolute temperatures T_1 and T_2 are mixed. There is no loss of energy. Find the temperature of the mixture if the masses of the molecules are m_1 and m_2 and the number of the molecules in the gases are n_1 and n_2 respectively.

The percentage by volume of C_(3)H_(8) in a gaseous mixture of C_(3)H_(8),CH_(4) and CO is 20. When 100mL of the mixture is burnt in excess of O_(2) the volume of CO_(2) produced is :

The vapour density of a maxture containing NO_2 and N_2 O_4 is 27.6 . The mole fraction of N_2 O_4 in the mixture is :

A solution containing H^(+) and D^(+) ions is in equilibrium with a mixture of H_(2) and D_(2) gases at 25^(@) C. If the partial pressures of both gases are 1.0 atm, find the ratio of [ H^(+) ] // [ D^(+) ] : (Given : E D^(+) /(D)=-0.003V and Ecell is =0.006V]

Under identical conditions of pressure and temperature, 4 L of gaseous moxture ( H_(2) and CH_(4) ) effuses through a hole in 5 min whereas 4 L of a gas X of molecular mass 36 takes to 10 min to effuse through the same hole. The mole ratio of H_(2):CH_(4) in the mixture is:

What is the molar mass of K2CO3.

A mixture of NH_4 NO_3 and (NH_4)_2 HPO_4 contain 30.40% mass per centof nitrogen. What is the mass ratio of the two components in the mixture ?