States of Matte...

A container contains equal mass of $$C{ O }_{ 2 },{ O }_{ 2 },C{ H }_{ 4 },S{ O }_{ 2 }$$ gases at a particular temperature.Which gas will exert the maximum amount of partial pressure?

The kinetic energy for 14 grams of nitrogen gas at $$127^0C$$ is nearly (mol. mass of nitrogen = 28 and gas constant = 8.31 $$JK^{-1} mol^{-1}$$)

If number of molecules of $$H_{2}$$ are double than that of $$O_{2}$$, then ratio of mean kinetic energy per molecule of hydrogen to that of oxygen at 300 K is:

An amount of 1.00 g of a gaseous compound of borbon and hydrogen occupies 0.820 liter at 1.00 atm and at $$3^{0}C$$. The compound is (R=0.0820 liter atm $$mole^{-10}K^{-1};$$ at. wt:H=1.0,B=10.8)

The gas Z in the above fraction is ?

Equal mass which of the following substance of occupy maximum volume at room temperature? 

Normal boiling point of a liquid is that temperature at which vapour of the liquid pressure of the liquid is equal to:

Two liquids A and B have $${P}_{A}^{o}$$ and $${P}_{B}^{o}$$ in the ratio $$1:3$$ and the ratio of number of moles of $$A$$ and $$B$$ in liquid phase are $$1:3$$. Then mole fraction of A in vapour phase in equilibrium with the solution is equal to:

Correct gas equation is :

Two flask $$A$$ and $$B$$ of equal volumes maintained temperature 300 K and 700 K contain equal mass of $$He(g)$$ and $$N_{2}(g)$$ respectively. What is the ratio of total translation kinetic energy of gas in flask $$A$$ to that of flask $$B$$?