If in the thermodynamic process shown in the figure, the work done by the system along A $\to$ B $\to$ C is 50 J and the change in internal energy during C $\to$ A is 30 J, then the heat supplied during A $\to$ B $\to$ C is:

         

1.	50 J	2.	20 J
3.	10 J	4.	80 J

The pressure in a monoatomic gas increases linearly from 4 atm to 8 atm when its volume increases from 0.2 m${}^3$ to 0.5 m${}^3$. The increase in internal energy will be:

The degree of freedom per molecule for a gas on average is 8. If the gas performs 100 J of work when it expands under constant pressure, then the amount of heat absorbed by the gas is:
1. 500 J
2. 600 J
3. 20 J
4. 400 J

An ideal gas is taken through the cycle \(A\rightarrow B\rightarrow C\rightarrow A\) as shown in the figure below. If the net heat supplied to the gas is \(10~\text{J}\), then the work done by the gas in the process \(B\rightarrow C\) is:

An ideal gas undergoes a cyclic process ABCA as shown. The heat exchange between the system and the surrounding during the process will be:

If the ratio of specific heat of a gas at constant pressure to that at constant volume is $\mathrm{\gamma }$, the change in internal energy of a mass of gas, when the volume changes from V to 2V at constant pressure, P is:

An ideal gas is taken through the process as shown in the figure. Then:

\(ABCA\) is a cyclic process. Its \(P\text-V\) graph would be:

1.		2.
3.		4.

In the \((P\text-V)\) diagram shown, the gas does \(5~\text J\) of work in the isothermal process \(ab\) and \(4~\text J\) in the adiabatic process \(bc.\) What will be the change in internal energy of the gas in the straight path from \(c\) to \(a?\) 

             
1. \(9~\text J\)
2. \(1~\text J\)
3. \(4~\text J\)
4. \(5~\text J\)

A horizontal cylinder has two sections of unequal cross-sections in which two pistons, A and B, can move freely. The pistons are joined by a string. Some gas is trapped between the pistons. If this gas is heated, the pistons will: