[" One mole of an ideal gas "(C_(v,m)=(5)/(2)R)" at "300K" and "5atm" is expanded adiabatically to a final pressure of "2" at "],[" against a constant pressure of "2atm" .Final temperature of the gas is: "],[[" (A) "270K," (B) "273K," (C) "248.5K," (D) "200K]]

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 :

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 .

300K a gas (gamma = 5//3) is compressed adiabatically so that its pressure becomes 1//8 of the original pressure. The final temperature of the gas is :

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.