`2m^(3)` volume of a gas at a pressure of `4xx10^(5) Nm^(-2)` is compressed adiabatically so that its volume becomes `0.5m^(3)` Find the new pressure . Compare this with the pressure that would result if the compression was isothermal. Calculate work done in each `gamma = 1.4`

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

The volume of a given mass of gas at NTP is compressed adiabatically to 1/5th of its original volume. What is the new pressure ? gamma =1.4.

300K a gas (gamma = 5//3) is compressed adiabatically so that its pressure becomes 1//8 of the original pressure. The final temperature of the gas is :

Diatomic gas at pressure 'P' and volume 'V' is compressed adiabatically to 1/32 times the original volume. Then the final pressure is

Diatomic gas at pressure 'P' and volume 'V' is compressed adiabatically to 1/32 times the original volume . Then the final pressure is

The initial volume of a gas is 2m^(3) . When the gas is compressed adiabatically at a pressure of 4 xx 10^(5) N cdot m^(-2) , its volume become 0.5 m^(3) . What will be the final pressure of the gas? If it is compressed isothermally, what will be the final pressure? Calculate the work done on the gas in both cases (gamma = 1.4) .

A volume of gas at atmospheric pressure is compressed adiabatically to half its original volume, Calculated the resulting pressure (gamma= 1.4).(1 atmoshpere = 0.76 m of mercury)