2 moles of an ideal diatomic gas `(C_(V)=5//2R)` at 300 K, 5 atm expanded irreversibly and adiabatically to a final pressure of 2 atm against a constant pressure of 1 atm.
(1) Calculate final temperature q, w, `DeltaH&DeltaU`
(2) Calculate corresponding values if the above process is carried out reversibly.

Two mole of ideal diatomic gas (C_("v,m")=5//2R) at 300 K and 5 atm expanded irreversly & adiabatically to a final pressure of 2 atm against a constant pressure of 1 atm. Calculate q, w, DeltaH&DeltaU .

Two mole of ideal diatomic gas (C_(v.m)= 5//2 R) at 300 K and 5 atm expanded irreversibly to a final pressue of 2atm against a constant pressue of 1 atm . Calculate q,w, DeltaH & DeltaU .

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

5mol of an ideal gas at 293K is expanded isothermally from an initial pressure 0.4 kPa to a final pressure of 0.1kPa against a constant external pressure of 0.1kPa . a. Calcualte q,w, Delta,U , and DeltaH . b. Calculate the corresponding value of q,w, DeltaU , and DeltaH if the above pressure is carried out reversibly.