In thermodynamic processes, which of the following statements is not true?

A polyatomic gas $\left(\gamma =\frac{{\displaystyle 4}}{{\displaystyle 3}}\right)$ is compressed to $\frac{1}{8}$ of its volume adiabatically. If its initial pressure is \(P_0,\) its new pressure will be:

Thermodynamic processes are indicated in the following diagram.
          
Match the following:

If an ideal gas undergoes two processes at constant volumes ${\mathrm{V}}_1$ $\mathrm{and}$ ${\mathrm{V}}_2$ as shown in the pressure-temperature (P-T) diagram, then:

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

2. ${\mathrm{V}}_1$ > ${\mathrm{V}}_2$

3. ${\mathrm{V}}_1$ < ${\mathrm{V}}_2$

4. ${\mathrm{V}}_1\ge {\mathrm{V}}_2$

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.

Which one of the following processes is reversible?

An ideal gas at \(27^{\circ}\mathrm{C}\) is compressed adiabatically to $\frac{8}{27}$ of its original volume. If $\gamma =\frac{5}{3}$, then the rise in temperature will be:
1. 450 K
2. 375 K
3. 225 K
4. 405 K

Can two isothermal curves cut each other?

A monoatomic gas at a pressure P, having a volume V, expands isothermally to a volume 2V and then adiabatically to a volume 16V. The final pressure of the gas is: (Take: γ= 5/3)

The initial pressure and volume of a gas are \(P\) and \(V\), respectively. First, it is expanded isothermally to volume \(4V\) and then compressed adiabatically to volume \(V\). The final pressure of the gas will be: [Given: \(\gamma = 1.5\)]