A diatomic molecule has how many degrees of freedom-
(1) 3 (2) 4 (3) 5 (4) 6
Mean kinetic energy per degree of freedom of gas molecules is:
1.
2. kT
3.
4.
A gas mixture consist of 2 moles of and 4 moles of Ar at temperature T. Neglecting all vibrational modes, the total internal energy of the system is:
(1)4RT
(2) 15RT
(3)9RT
(4)11RT
Which one of the following gases possesses the largest internal energy?
1. | 2 moles of helium occupying 1m3 at 300 K |
2. | 56 kg of nitrogen at \(10^5 \mathrm{Nm}^{-2}\) and 300 K |
3. | 8 grams of oxygen at 8 atm and 300 K |
4. | \(6 \times 10^{26}\) molecules of argon occupying 40 m3 at 900 K |
The degrees of freedom of a triatomic gas is
1. 2
2. 4
3. 6
3. 8
The number of translational degrees of freedom for a diatomic gas is
1. 2
2. 3
3. 5
4. 6
Two ideal gases at absolute temperature and are mixed. There is no loss of energy. The masses of the molecules are and and the number of molecules in the gases are and respectively. The temperature of mixture will be
1.
2.
3.
4.
A vessel contains a mixture of one mole of oxygen and two moles of nitrogen at \(300\) K. The ratio of the average rotational kinetic energy per molecule to that per molecule is:
1. | 1 : 1 |
2. | 1 : 2 |
3. | 2 : 1 |
4. | depends on the moments of inertia of the two molecules |
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 |
Assertion The molecules of a monoatomic gas have three degrees of freedom.
Reason The molecules of a diatomic gas have five degrees of freedom.