Thermodynamics (Physics)

A real gas within a closed chamber at 27 undergoes the cyclic process as shown in figure. The gas obeys PV3 = RT equation for the path A to B. The net work done in the complete cycle is (assuming R = 8 J/mol K): [figure]

1. -20 J
2. 205 J
3. 225 J
4. 20 J

Two different adiabatic paths for the same gas intersect two isothermal curves as shown in P-V diagram. The relation between the ratio VaVd and the ratio VbVc is: [figure]

1. VaVd VbVc
2. VaVd = ( VbVc )-1
3. VaVd = VbVc
4. VaVd = ( VbVc )2

A diatomic gas ( = 1.4) does 100 J of work in an isobaric expansion. The heat given to the gas is :

1. 150 J
2. 490 J
3. 350 J
4. 250 J

The specific heat at constant pressure of a real gas obeying PV2 = RT equation is:

1. R
2. CV + R
3. CV + R2V
4. R3 + CV

A total of 48 J heat is given to one mole of helium kept in a cylinder. The temperature of helium increases by 2 C. The work done by the gas is: Given, R = 8.3 J K-1 mol-1.

1. 23.1 J
2. 48 J
3. 24.9 J
4. 72.9 J

The heat absorbed by a system in going through the given cyclic process is : [figure]

1. 61.6 J
2. 431.2 J
3. 19.6 J
4. 616 J

During an adiabatic process, if the pressure of a gas is found to be proportional to the cube of its absolute temperature, then the ratio of CPCV for the gas is :

1. 53
2. 32
3. 75
4. 97

A sample of gas at temperature T is adiabatically expanded to double its volume. Adiabatic constant for the gas is = 3/2. The work done by the gas in the process is: ( = 1 mole)

1. RT[2 2 - 1]
2. RT[2 - 2]
3. RT[1 - 2 2]
4. RT[ 2 - 2]

The pressure and volume of an ideal gas are related as PV3/2 = K (Constant). The work done when the gas is taken from state A (P1, V1, T1 ) to state B (P2, V2, T2 ) is :

1. 2 (P2 V2 - P1 V1 )
2. 2 ( P1 V1 - P2 V2 )
3. 2 (P2V2 - P1V1 )
4. 2 (P1V1 - P2V2 )

A diatomic gas ( =1.4) does 200 J of work when it is expanded isobarically. The heat given to the gas in the process is :

1. 800 J
2. 600 J
3. 700 J
4. 850 J