A diatomic gas at pressure P and volume V is compressed adiabatically to `frac(1)(32)` times the original volume. Find the final pressure.

A monatomic gas at a pressure P, having a volume V expands isothermally to a volume 2 V and then adiabatically to a volume 16 V. The final pressure of the gas is ( take gamma=5/3 )

An ideal gas of volume 1.0L is adiabatically compressed to frac(1)(15)th of its initial volume. Its initial pressure and temperature is 1.01xx10^5Pa and 275^@C respectively. Given Cv for ideal gas = 20.8J/mol.K and gamma = 1.4. Calculate final pressure.

An ideal gasin a cylinder is compressed adiabatically to one-third its original volume. During the processif 45 J of work is done on the gas by the compressing agent, what is the change in internal energy?

An ideal gas of volume 1.0L is adiabatically compressed to frac(1)15)th of its initial volume. Its initial pressure and temperature is 1.01xx10^5 Pa and 275^@C respectively. Given Cv for ideal gas = 20.8J/mol.K and gamma = 1.4. Calculate final temperature

An ideal gas of volume 1.0L is adiabatically compressed to frac(1)15)th of its initial volume. Its initial pressure and temperature is 1.01xx10^5 Pa and 275^@C respectively. Given Cv for ideal gas = 20.8J/mol.K and gamma = 1.4. How would your answers change, if the process were isothermal?

If gamma=2.5 and volume is equal to (1)/(8) times to the initial volume then perssure p' is equal to (initial pressure = p)

Two moles of an ideal monatomic gas occupies a volume V at 27 °C. The gas expands adiabatically to a volume 2V. Calculate (i) the final temperature of the gas and (ii) change in its internal energy.

The product of the pressure and volume of an ideal gas is

Two samples A and B of a gas initially of the same temperature and pressure are compressed from a volume V to a volume frac(V)(2) such that A is compressed isothermally and B adiabatically. The final pressure of