Compare the partial pressures of gases A and B when 3 moles of A and 5 moles of B mixed in constant volume, and `25^(@) C` and 1 atm pressure.

Calculate the partial pressures of O_2 and H_2 in a mixture of 3 moles of O_2 and 1 mole of H_2 at S.T.P.

Calculate the partial pressures N_2 and H_2 in a mixture of two moles of N_2 and two moles of H_2 at STP.

How many moles of helium gas occupy 22.4L at O^@C and 1 atm pressure ?

Derive the relationship between partial pressure of gas and its mole fraction.

310 J of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 25^(@)C to 35^(@)C .The amount of heat required to raise the temperature of the gas through the same range at constant volume is

A 300 K the vapour pressure of an ideal solution containing 1 mole of liquid A and 2 moles of liquid B is 500 mm of Hg. The vapour pressure of the solution increases by 25 mm of Hg if one more mole of B is added to the above ideal solution at 300 K. Then vapour pressure of A in its pure state is :

Two liquids A and B form an idea solution. What will be the vapour pressure at 27^(@)C of a solution having 1.5 mol of A and 4.5 mol of B ? The vapour pressure of A and B at 27^(@)c is 0.116 atm and 0.140 atm , respectively.

Estimate the total number of air molecules in a room capacity 25m^(3) at a temperature of 27^(@)C and 1 atm pressure.

What will happen to the volume of a bubble of air found under water in a lake, where the temperature is 15^(@)C and the pressure is 1.5 atm. If the bubble then rises to the surface where the temperature is 25^(@)C and the pressure is 1.0 atm ?