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

A thermodynamic system undergoes a cyclic process \(ABCDA\) as shown in Fig. The work done by the system in the cycle is: 
             
1. \( P_0 V_0 \)
2. \( 2 P_0 V_0 \)
3. \( \frac{P_0 V_0}{2} \)
4. zero

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

1.		2.
3.		4.

In the cyclic process shown in the pressure-volume \((P-V)\) diagram, the change in internal energy is equal to:

1. $\pi {\left(\frac{{\mathrm{P}}_2-{\mathrm{P}}_1}{2}\right)}^2$

2. $\mathrm{\pi }{\left(\frac{{\mathrm{V}}_2-{\mathrm{V}}_1}{2}\right)}^2$

3. $\frac{\mathrm{\pi }}{4}({\mathrm{P}}_2-{\mathrm{P}}_1)({\mathrm{V}}_2-{\mathrm{V}}_1)$

4. zero

Which one of the following is correct for one complete cycle of a thermodynamic process on a gas as shown in the \((P-V)\) diagram?

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:

For the indicator diagram given below, which of the following is not correct?

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. \(5~\text J\)

In a cyclic process, the internal energy of the gas:

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: