Which of the following graph shows the variation of pressure P with volume V for an ideal gas at a constant temperature?

1.		2.
3.		4.

A gas performs the minimum work when it expands:

An ideal gas goes from A to B via two processes, l and ll, as shown. If $∆{\mathrm{U}}_1$ and $∆{\mathrm{U}}_2$ are the changes in internal energies in processes I and II, respectively, then (\(P:\) pressure, \(V:\) volume)

An ideal monoatomic gas \(\left(\gamma = \frac{5}{3}\right )\) absorbs 50 cal in an isochoric process. The increase in internal energy of the gas is:

The pressure-temperature (P-T) graph for two processes, A and B, in a system is shown in the figure. If ${\mathrm{W}}_1$ and ${\mathrm{W}}_2$ are work done by the gas in process A and B respectively, then:

1. ${\mathrm{W}}_1$ = ${\mathrm{W}}_2$

2. ${\mathrm{W}}_1$ < ${\mathrm{W}}_2$

3. ${\mathrm{W}}_1$ > ${\mathrm{W}}_2$

4. ${\mathrm{W}}_1$ = - ${\mathrm{W}}_2$

The variation of molar heat capacity at constant volume ${\mathrm{C}}_{\mathrm{V}}$ with temperature T for a monatomic gas is:

1.		2.
3.		4.

When a system is moved from state a to state b along the path acb, it is discovered that the system absorbs 200 J of heat and performs 80 J of work.  Along the path adb, heat absorbed Q = 144 J. The work done along the path adb is:

Heat is supplied to a diatomic gas in an isochoric process. The ratio $∆\mathrm{Q}:\hspace{0.17em}∆\mathrm{U}$ is: (symbols have usual meanings)

1. 5 : 3

2. 5: 2

3. 1: 1

4. 5: 7

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

The work done by an ideal diatomic gas in its sudden expansion is 20 J. The change in the internal energy of the gas will be:

1. 20 J

2. 0 J

3. $-20$ J

4. $-15$ J