A gas originally at `1.10atm` and `298K` underwent a reversible adiabatic expansion to `1.00atm` and `287K`. What is the molar heat capacity of the gas?

A perfect gas undergoes a reversible adiabatic expansion from (300 K, 200 atm) to (90 K, 10 atm). Find the atomicity of gas.

A perfect gas undergoes a reversible adiabatic expansion from (300 K, 200 atm) to (90 K, 10 atm). Find the atomicity of gas.

Which gas is most dense at 1 atm and 298 K ?

1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?

1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?

One mol of an ideal diatomic gas underwent an adiabatic expansion form 298K, 15.00atm , and 5.25L to 2.5atm against a constant external pressure of 1.00atm . What is the final temperature of the system?

One mol of an ideal diatomic gas underwent an adiabatic expansion form 298K, 15.00atm , and 5.25L to 2.5atm against a constant external pressure of 1.00atm . What is the final temperature of the system?

A sample of 3.0 mole of perfect gas at 200 K and 2.0 atm is compressed reversibly and adiabatically until the temperature reaches 250 K . Given that molar heat capacity at 27.5 J K^(-1) mol^(-1) at constant volume calculate q,W,DeltaU,DeltaH and the final pressure and volume.