26165.If P is the exerted by a gas and E is the K.E. per unit volume, then
P = $\dfrac{\text{E}}{3}$
P = $\dfrac{\text{E}}{3}$
P = $\dfrac{\text{2E}}{3}$
P = $\dfrac{3}{\text{2E}}$
26166.A gas at a pressure P0 is contained in a vessel. If the masses of all the molecules are halved and their velocities doubled, the resulting pressure P would be equal to
4 P0
2 P0
P0
P0 / 2
26167.The temperature of a gas is raised from 27°C to 927°C. the root mean square speed
$\sqrt{\dfrac{927}{27}}$ times the earlier value
Gets halved
Remains the same
Gets doubled
26169.A gas in a container A is in thermal equilibrium with another gas of the same mass in container B. if we denote the corresponding pressures and volumes by the suffices A and B, then which of the following statement is most likely to be true
PA = PB, VA = VB
PA ≠ PB, VA = VB
$\dfrac{\text{P}_A}{\text{P}_B} = \dfrac{\text{V}_A}{\text{V}_B}$
PA VA = PB VB
26170.Boyl’s law is applicable in,
Isochoric process
Isothermal process
Isobaric process
Isotonic process
26171.Real gases show markable deviation from that of ideal gas behavior at
High temperature and low pressure
Low temperature and high pressure
High temperature and high pressure
Low temperature and low pressure
26172.If the pressure of an ideal gas is decreased by 10% isothermally, then its volume will
Increase by 10%
Increase by 11.1%
Decrease by 10%
Decrease by 9%
26173.One any planet, the presence of atmosphere implies [νrms = root mean square velocity of molecules and νe = escape velocity]
vrms << ve
vrms > ve
vrms = ve
vrms = 0
26174.One mole of an ideal gas requires 207 J heat to raise the temperature by 10 K, when heated at constant pressure. If the same gas is heated at constant volume to raise the temperature by 10K, then heat required is
96.6 J
124 J
198.8 J
215.4 J
26175.Which of the following properties of gas molecule the one that is same for all ideal gases at a particular temperature is
Mass
Velocity
Momentum
Kinetic energy
26177.At constant volume temperature is increased then
Collision on walls will be less
Collision frequency will be increases
Collision will be in straight line
Collision will not change
26178.N molecules, each of mass m, of gas A and 2 N molecules, each of mass 2 m, of gas B are contained in the same vessel which maintained at a temperature T. the mean square of he velocity of molecules of B type is denoted by v2 and the mean square of the X component of the velocity of A type is denoted by ω2, then $\left(\dfrac{\omega^2}{v^2}\right)$ is
2
1
$\dfrac{1}{3}$
$\dfrac{2}{3}$
26179.Consider a gas with density ρ and C as the root mean square velocity of its molecules contained in a volume. If the system moves as a whole with velocity ν, then the pressure exerted by the gas is
$\dfrac{1}{3}\rho C^2$
$\dfrac{1}{3}\rho (C + v)^2$
$\dfrac{1}{3}\rho (C - v)^2$
$\dfrac{1}{3}\rho (C^2 - v^2)$
26180.The r.m.s velocity of oxygen molecules at 27°C is 318 m/s. the r.m.s velocity of hydrogen molecules at 127°C is
1470 m/s
1603 m/s
1869 m/s
2240 m/s
26181.By what percentage should the pressure of a given mass of a gas be increased so as to decrease its volume by 10% at a constant temperature?
8.1%
9.1%
10.1%
11.1%
26182.The equation of state corresponding to 8 g of O2 is,
$PV = \dfrac{\text{RT}}{\text{2}}$
$PV = \dfrac{\text{RT}}{\text{4}}$
PV = RT
PV = 8RT
26183.Three containers of the same volume contains three different gases. The masses of the molecules are m1, m2 and m3 and number of molecules in their respective container are N1, N2 and N3, the gas pressure in the container are P1, P2, and P3 respectively. All the gasses are now mixed and put in one of these containers. The pressure P of the mixture is
P < (P1 + P2 + P3)
$\text{P} = \dfrac{\text{P}_1 + \text{P}_2 + \text{P}_3}{3}$
P = (P1 + P2 + P3)
P > (P1 + P2 + P3)
26184.According to kinetic theory of gases, at absolute zero of temperature
Water freezes
Liquid helium freezes
Molecular motion stops
Liquid hydrogen freezes