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 :

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 .

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//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 .

Four moles of an ideal diatomic gas (gamma = 1.4) at 300 K and 12 atm expanded irreversibly & adiabatically to a final pressure of 2.4 atm against a constant pressure of 2 atm . Calcualate W & DeltaH (magnitude only) . Report your answer as (|X + Y|)/(10) , where W = X xx 10R, DeltaH = Y xx 10R and R is gas constant.