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

Consider two containers A and B containing identical gases at the same pressure, volume and temperature. The gas in container A is compressed to half of its original volume isothermally while the gas in container B is compressed to half of its original value adiabatically. The ratio of final pressure of gas in B to that of gas in A is

A litre of hydrogen at 27^@C and 10^5 Nm^-2 pressure expand isothermally until its volume is doubled and then adiabatically until its volume is redoubled. Find the final pressure of the gas. 1(gamma = 1.4)

At a given volume and temperature, the pressure of a gas:

An ideal gas with pressure P, volume V and temperature T is expanded isothermally to a volume 2V and a final pressure P_i , If the same gas is expanded adiabatically to a volume 2V and a final pressure P_alpha find the value of ratio P_alpha/P_i . The ratio of the specific heats for the gas is 1.67.

What is heat capacity at constant volume and at constant pressure ?

A gas occupying one litre at 80 cm pressure is expanded adiabatically to 1190 cc.If the pressure falls to 60 cm in the process ,deduce the value of gamma .

When one mole of an ideal gas is compressed to half of its initial volume and simultaneously heated to twice its initial temperature, the change in entropy of gas (Delta S) is:

A vessel of 120 mL capacity is containing a certain mass of gas at 20^(@)C and 750 mm pressure. The gas was transferred to a vessel, whose volume is 180 ml. Calculate the pressure of the gas at 20^(@)C .