A tyre is pumped to a pressure of 3.375 atmospheres and at `27^@C` suddently bursts.What is the final temperature?`(gamma=1.5)`.

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

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.

A compressed cylinder of gas contains 1.50xx10^(3) g of N_(2) gas at a pressure of 2.0xx10^(7) Pa and a temperature of 17.1^(@)C . What volume of gas has been released into the atmosphere if the final pressure in the cylinder is 1.80xx10^(5) Pa ? Assume ideal behaviour and that the gas temperature is unchanged.

Starting out on a trip into the mountains, you inflate the tires on your automobile to a recommended pressure of 3.21xx10^(5) Pa on a day when the temperature is - 5.0^(@)C . You drive to the beach, where the temperature is 28.0^(@)C . Assume that the volume of the tire has increased by 3%. What is the final pressure in the tyres?

A vessel is filled with an ideal gas at a pressure of 20 atm is at a temperature of 27^@ C . One half of the mass is removed from the vessel and the temperature of the remianing gas is increated to 87^@C . What will be the pressure at this temperature?

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?

Calculate the pressure exerted by two moles of gas at 27^@C in a 1 litre flask.

An oxygen cylinder of volume 30 litres has an initial gauge pressure of 15 atm and a temperature of 27 ^@C . After some oxygen is withdrawn from the cylinder, the gauge pressure drops to 11 atm and its temperature drops to 17 ^@C . Estimate the mass of oxygen taken out of the cylinder ( R= 8.31 J mol^-1 K^-1 ’, molecular mass of O_2 = 32 u)

A volume of gas at atmospheric pressure is compressed adiabatically to half its original volume. Calculate the resulting pressure (gamma = 1.4)