Two samples of a gas initially at same temperature and pressure are compressed from a volume `V` to ` (V)/(2)` . One sample is compressed isothermally and the other adiabatically . In which sample is the pressure greater?

Two samples A and B of a gas are initially at the same temperature and pressure are compressed from volume V_1 to V/2 (A isothermally and B adiabatically). The final pressure is

Two samples A and B of a certain gas, which are initially at the same temperature and pressure, are compressed from volume V to V /2. A is compressed isothermally, while Bis compressed adiabatically. The final pressure of A is

Two sample A and B of a gas initially at the square at the same pressure and temperature are compressed from volume V to V//2 (A isothermally and B adiabatically). The final pressure of A is

A mono-atomic gas X and an diatomic gas gamma both initially at the same temperature and pressure are compressed adiabatically from a volume V to V//2 . Which gas will be at higher temperature?

Initially two gas samples 1 and 2 are at the same condition. The volume of the two are halved, one isothermally and the other adiabatically. What is the relation between the final pressures p_(1) and p_(2) ?

A certain mass of an ideal gas is at pressure P_(1) and volume V_(1) . If is compressed isothermally and then allowed to expand adiabatically untill its pressure returns to P_(1) . The gas is then allowed to expand its original volume. Which of the following P -V graphs are these process correctly shown?

Statement-1: Two gases at same pressure, volume & temperature are compressed to same volume. The first isothermally and second adiabatically, greater work is done on the gas for an adiabatic process. Statement-2: Final temperature for gas going under isothermal process is more than gas going under adiabatic process.