If an oxygen atom and hydrogen atom are having the same temperature, then ratio of their average kinetic energy is
1 : 1
2 : 1
4 : 1
1 : 4
The temperature of H2 at which the rms velocity of its molecules is seven times the rms velocity of the molecules of nitrogen at 300 K is:
2100 K
1700 K
1350 K
1050 K
A gas mixture consists of 2 moles of oxygen and 4 moles of argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is:
4 RT
9 RT
11 RT
15 RT
Three perfect gases at absolute temperatures T1, T2, and T3 are mixed. The masses of molecules are m1, m2, and m3 and the number of molecules are Tn1, n2, and n3 respectively. Assuming no loss of energy, the final temperature of the mixture is:
A gas at a temperature of 250 K is contained in a closed vessel. If the gas is heated through 1 K, then percentage increase in its pressure is
0.1 %
0.2 %
0.3 %
0.4 %
R.M.S velocity of a molecule is C at pressure P. If pressure is increased two times, then r.m.s velocity becomes
0.5 C
C
2 C
3 C
The relation between pressure P and average kinetic energy E per unit volume of a gas is:
P=2E/3
P=E/3
P=3E/2
P=3E
The relation PV=RT can describe behavior of a real gas at :
High temperature and high density
High temperature and low density
Low temperature and low density
Low temperature and high density
From the following statements concerning ideal gas at any given temperature T, select the correct one(s) :
The co-efficient of volume expansion at constant pressure is the same for all ideal gases.
The average translational kinetic energy per molecule of oxygen gas is 3 kT, k being Boltzmann constant
The mean-free path of molecules increases with increases in the pressure.
In a gaseous mixture, the average translational kinetic energy of the molecules of each component is different.
A diatomic gas initially at 180 C is compressed adiabatically to one eighth of its original volume. The temperature after compression will be:
180 C
395.40 C
887.40 C
1140 C
