A certain mass of gas is allowed to expand adiabatically to 6 times its original volume. Find the relation between the initial and final pressure. `gamma=1.4`.

An ideal gas at 27^@C and a pressure of760 mm of mercury is compressed isotiiermally until its volume is halved. It is then expanded adiabatically to twice its original volume. If the value of gamma for the gas is 1.4. Calculate the final pressure and temperature of the gas.

Air initially under a pressure of 10^5N//m^2 is compressed adiabatically to 1//16 times its original in a diesel engine. Calculate the work done in the process. gamma_(air) =1.4

Calculate the final temperature when a given mass of a gas at 0^@C is suddenly compressed adiabatically to a pressure 20 times the initial pressure gamma=1.42

One gm mole of an ideal gas at S.T.p is subjected to a reversible adiabatic expansion to double its. volume Find the change in internal energy in the process. Given =gamma=1.4 .

1 mole of an ideal gas at 25^@C is subjected to expand reversibly ten times of its intial volume. The change in entropy of expansion is:

Two identical samples of gas are allowed to expand to double it’s volume, one adiabatically and the other isothermally. In which case more work is done ?

One gram mole of oxygen gas at 127^@C expands isothermally until its volume is doubled. Find the amount of work done and heat produced R=8.314"jmole"^-1k^-1

A gas is heated from 0^@ C to 100^@ C at 1.0 atm pressure. If the initial volume of the gas is 10 litre, its final volume would be :

Ten litres of dry air at 27^@C and 76 cm pressure is compressed adiabatically to a volume of 03 liter. Assuming gamma = 1.4 for dry air, fine the resulting pressure and temperature.