Ideal gas is taken through cycle $P\to Q\to R\to P$ as shown in the figure. If net heat supplied to the gas in the cycle is 15 J, the work done by the gas in the process $R\to P$ is

1. 5J

2. -15 J

3. -20 J

4. -12 J

Internal energy remains the same throughout the process along the path in

1 Adiabatic process

2 Isothermal process

3 Cyclic process

4 Both (2) & (3)

The cyclic process of \(2\) moles of diatomic gas is shown in the figure. Which of the following statements is correct?

Without external heat work done possible in

1 Adiabatic process

2 Isochoric process

3 Isothermal process

4 Isobaric process

The PV diagram of an ideal gas is shown in the figure. The work done by the gas in the process $1\to 2\to 3\to 4$ is given by:

Given below are two statements:

Which of the following is true for the molar heat capacity of an ideal gas?

An ideal gas undergoes a cyclic process as shown in the graph between pressure \((P)\) and temperature \((T).\) The part of the graph which represents the absorption of heat from the surrounding are:

1. \(\text{AB, CD}\)
2. \(\text{DA, BC}\)
3. \(\text{DA, AB}\)
4. \(\text{BC, AB} \)

During an adiabatic process, the pressure of a gas is found to be proportional to the fourth power of its absolute temperature. The ideal gas would be :

1.  ${\mathrm{H}}_2$

2.  He

3.  The mixture of ${\mathrm{H}}_2$ and He

4.  ${\mathrm{CH}}_2$

The pressure of a monoatomic gas increases linearly from $4\times {10}^5$ N/m² to $8\times {10}^5$ N/m² when its volume increases from 0.2 m³ to 0.5 m³. The molar heat capacity of the gas is:
[R = 8.31 J/mol k]  

1. 20.1 J/molK               

2. 17.14 J/molK

3. 18.14 J/molK                                   

4. 20.14 J/molK