A gas occupies 200mL at a pressure of 0.820 bar at 20 o C. How much volume will it occupy when it is subjected to external pressure of 1.025 bar at the same temperature?

At 27^(@)C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth of the original value at the same temperature ?

The decomposition of ammonia on tungsten surface at 500 K follows zero order kinetics. The half-life period of this reaction is 45 minutes when the initial pressure is 4 bar. The half life period (minutes) of the reaction when the initial pressure is 16 bar at the same temperature is

A sample of nitrogen gas occupies a volume of 1.0L at a pressure of 0.5 bar and at 40∘C. Calculate the pressure the gas if compressed to 0.225ml at −6∘C

At what pressure a quantity of gas will occupy a volume of 60 mL, if it occupies a volume of 100mL at a pressure of 720 mm (while temperature is constant) :

A certen amount of gas at 2.5^(@)C and at a pressure of 0.80 atm is kept in a glass vessel. Suppose that the vessel can withstand a pressure of 2.0 atm. How high can you raise the temperature of the gas without bursting the vessel?

A gas occupies a volume of 250 ml at 745 mm Hg and 25 ∘ C. What additional pressure is required to reduce the gas volume to 200 ml at the same temperature?

Calculate volume occupied by two moles of gas at 27^@C and under a pressure of 1 atmosphere.

At 300 K, 36 g of glucose present in a litre of its solution has an osmotic pressure of 4.98 bar. If the osmotic pressure of the solution is 1.52 bars at the same temperature, what would be its concentration?

10 litre of a non linear polyatomic ideal gas at 127^(@)C and 2 atm pressure is suddenly released to 1 atm pressure and the gas expanded adiabatically against constant external pressure. The final temperature and volume of the gas respectively are.

The vapour pressure of water at 293K is 0.0231 bar and the vapour pressure of a solution of 108.24 g of a compound in 1000 g of water at the same temperature is 0.0228 bar. Calculate the molar mass of the solute.