Two non-reacting gases `CH_4` of mass 6.4g and `CO_2` of mass 8.8g is mixed in a vessel of volume 10litre at `27^@C` . the pressure in KPa is?

8g of oxygen, 14 g of nitrogen and 22 g carbon dioxide are mixed in an encloser of volume 10 litre and temperature 27^(@)C . Calculate the pressure exerted by the mixture , R= 8.3 J "mole"^(-1)K^(-1) , Molecular weight of oxygen , nitrogen and carbon 32 , 28 and 44 respectively.

A mixture containing 1.6 g of O_(2) , 1.4 g of N_(2) and 0.4 g of He occupies a volume of 10 litres at 27^(@)C . Calculate the total pressure of the mixutre and partial pressure of each compound.

In what ratio by mass, the gases CO and 2 butene (C_4 H_8) be mixed in a vessel so that they cause same partial pressures ?

The pressure exerted by a non-reactive gaseous mixture of 6.4g of methane and 8.8 g of carbon dioxide in a 10L vessel at 27^(@)C is "__________" kPa. ( Round off to the Nearest Integer ). [ Assume gases are ideal, R = 8.314] mol^(-1) K^(-1) Atomic masses : C : 120 u, H : 1.0 u, O : 16.0 u ]

2.8 g of N_(2) 0.40 g of H_(2) and 6.4 g of O_(2) are placed in a container of 1.0 L capacity at 27^(@) C. The total pressure in the container is

Two gases A and B have molecular weight 60 and 45. 0.6 g of A and 0.9 g of B are mixed in a closed vessel. Total pressure is 720 mm. The partial pressure of A is