1. | \(\dfrac{4+3\gamma}{\gamma-1}\) | 2. | \(\dfrac{3+4\gamma}{\gamma-1}\) |
3. | \(\dfrac{4-3\gamma}{\gamma-1}\) | 4. | \(\dfrac{3-4\gamma}{\gamma-1}\) |
The value \(\gamma = \dfrac{C_P}{C_V}\) for hydrogen, helium, and another ideal diatomic gas \(X\) (whose molecules are not rigid but have an additional vibrational mode), are respectively equal to:
1. | \(\dfrac{7}{5}, \dfrac{5}{3}, \dfrac{9}{7}\) | 2. | \(\dfrac{5}{3}, \dfrac{7}{5}, \dfrac{9}{7}\) |
3. | \(\dfrac{5}{3}, \dfrac{7}{5}, \dfrac{7}{5}\) | 4. | \(\dfrac{7}{5}, \dfrac{5}{3}, \dfrac{7}{5}\) |
A gas mixture consists of \(2\) moles of \(O_2\) and \(4\) moles of \(Ar\) at temperature \(T.\) Neglecting all the vibrational modes, the total internal energy of the system is:
1. | \(15RT\) | 2. | \(9RT\) |
3. | \(11RT\) | 4. | \(4RT\) |
One mole of an ideal diatomic gas undergoes a transition from \(A\) to \(B\) along a path \(AB\) as shown in the figure.
The change in internal energy of the gas during the transition is:
1. | \(20\) kJ | 2. | \(-20\) kJ |
3. | \(20\) J | 4. | \(-12\) kJ |
To find out the degree of freedom, the correct expression is:
1.
2.
3.
4.