Calculate the final pressure of a sample of carbon dioxide that expands reversibly and adiabatically from `57.4kPa` and `1.0` to a final volume of `2.0L` . Take `gamma = 1.4`

Calculated the final temprature (in Kelvin of a sample of argon of mass 12.0 g that is expanjded reversibly and adiabatically from 1.0 L at at 273 K to 3.0 L. (Take : 3sqrt9=2.08 )

Calculate the final temperature of a monoatomic ideal gas that is compressed reversible and adiabatically from 16L to 2L at 300 K :

Calculate the final temperature of a monoatomic ideal gas that is compressed reversible and adiabatically from 16L to 2L at 300 K :

Calculate the final temperature of a monoatomic idal gas that is compressed reversible and adiabatically from 16L to 2L at 300 K :

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

A sample of carbon dioxide of mass 2.45 g at 27.0^(@) C is allowed to expand reversibly and adiabatically from 500 mL to 3.00 L What is the work done by the gass ? Take: (6)^(0.4)=2,R=(25)/(3)J//mol//K]

A sample of ideal gas undergoes isothermal expansion in a reversible manner from volume V_(1) to volume V_(2) . The initial pressure is P_(1) and the final pressure is P_(2) . The same sample is then allowed to undergoes reversible expansion under adiabatic conditions from volume V_(1) to V_(2) . The initial pressure being same but final pressure is P_(2) . Which relation is correct (gamma = (C_(P))/(C_(V))) ?