JEE Questions for Physics Kinetic Theory Of Gases Quiz 3 - MCQExams.com

The root mean square speed of hydrogen molecules of an ideal hydrogen kept in a gas chamber at 0o C is 3180 ms–1. The pressure on the hydrogen gas is (Density of hydrogen gas is 8.99 × 10–2 kg/m3, 1 atm = 1.01 × 105 Nm–2
  • 1.5 atm
  • 1.0 atm
  • 3.0 atm
  • 2.0 atm
A cylinder of capacity 20 litres is filled with H2 gas. The total average kinetic energy of translatory motion of its molecules is 1.5 × 105 J. The pressure of hydrogen in the cylinder is
  • 4 × 106 Nm–2
  • 3 × 106 Nm–2
  • 5 × 106 Nm–2
  • 2 × 106 Nm–2
The average kinetic energy per molecule of a gas at –23o C and 75 cm pressure is 5 × 10–14 erg for H2. The mean kinetic energy per molecule of the O2 at 227o C and 150 cm pressure will be

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    Physics-Kinetic Theory of Gases-75338.png

  • Physics-Kinetic Theory of Gases-75339.png

  • Physics-Kinetic Theory of Gases-75340.png
The ratio of mean kinetic energy of hydrogen and nitrogen at temperature 300 K and 450 K respectively is
  • 2:3
  • 3:2
  • 4:9
  • 2:2
Pressure of an ideal gas is increased by keeping temperature constant what is the effect on kinetic energy of molecules.
  • Decrease
  • Increase
  • No change
  • Can`t be determined
A sealed container with negligible co-efficient of volumetric expansion contains helium (a monoatomic gas) when it is heated from 200 K to 600 K, the averagy K.E. of helium atom is
  • Halved
  • Doubled
  • Unchanged
  • Increased by factor √2
The mean kinetic energy of a gas at 300 K is 100J. mean energy of the gas at 450 K is equal to
  • 100 J
  • 150 J
  • 3000 J
  • 450 J
The average kinetic energy of a gas molecule at 27o C is 6.21 × 10–21 J. Its average kinetic energy at 227o C will be

  • Physics-Kinetic Theory of Gases-75344.png
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    Physics-Kinetic Theory of Gases-75345.png

  • Physics-Kinetic Theory of Gases-75346.png

  • Physics-Kinetic Theory of Gases-75347.png
The average translational kinetic energy of O2 (molar massmolecules at a particular temperature is 0.068 eV. The translational kinetic energy of N2 (molar massmolecules in eV at the same temperature is
  • 0.003 eV
  • 0.068 eV
  • 0.056 eV
  • 0.678 eV
The kinetic energy of one mole gas at 300 K temperature is E. At 400 K temperature kinetic energy is E\'. The value of E\'/E is
  • 2
  • 16/9
  • 1.33

  • Physics-Kinetic Theory of Gases-75349.png
The temperature at which the average translational kinetic energy of a molecule is equal to the energy gained by an electron accelerating from rest through a potential differencc of 1 volt is

  • Physics-Kinetic Theory of Gases-75351.png
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    Physics-Kinetic Theory of Gases-75352.png

  • Physics-Kinetic Theory of Gases-75353.png

  • Physics-Kinetic Theory of Gases-75354.png
According to the kinetic theroy of gases the r.m.s velocity of gas molecules is directly proportional to

  • Physics-Kinetic Theory of Gases-75356.png
  • 2)
    Physics-Kinetic Theory of Gases-75357.png
  • T

  • Physics-Kinetic Theory of Gases-75358.png
If the ratio of vapour density for hydrogen and oxygen is 1/16 then under constant pressure the ratio of their rms velocities will be
  • 4:1
  • 1:16
  • 16:1
  • 1:4
To what temperature should the hydrogen at 327o C cooled at constant pressure, so that the root mean square velocity of its molcules become half of its previous value
  • –100o C
  • 123o C
  • 0o C
  • –123o C
At what temperature is the root mean square velocity of gaseous hydrogen molecules equal to that of oxygen molecules at 47o C?
  • –73 K
  • 80 K
  • 20 K
  • 3 K
When temperature of an ideal gas is increased from 27o C to 227o C, its rms speed changed from 400 ms–1 to Vs. The Vs is
  • 516 ms–1
  • 746 ms–1
  • 310 ms–1
  • 450 ms–1
The rms speed of the molecules of a gas at a pressure 105 Pa and temperature 0o C is 0.5 km/s. If the pressure is kept constant but temperature is raised to 819o C, the rms speed becomes
  • 1.5 kms–1
  • 2 kms–1
  • 1 kms–1
  • 5 kms–1
The root mean square velocity of a gas molecule of mass m at a given temperature is proportional to
  • mo
  • m–1/2
  • m1/2
  • m
The ratio of the vapour densities of two gases at a given temperature is 9:8, The ratio of the rms velocities of their molecule is
  • 2:3√2
  • 2√2 : 3
  • 9:8
  • 8:9
For a gas, the rms speed at 800 K is
  • Four times the value at 200 K
  • Twice the value at 200 K
  • Half the value at 200 K
  • same as at 200 K
The temperature of an ideal gas is increased from 27o C to 927o C. The root mean square speed of its molecules becomes
  • Four times
  • One-fourth
  • Half
  • Twice
At a given temperature the root mean square velocities of Oxygen and hydrogen molecules are in the ratio
  • 1:4
  • 1:16
  • 16:1
  • 4:1
If mass of He atom is 4 times that of hydrogen atom, then rms speed of the is
  • Two times of H – vrms speed
  • Four times of H – vrms speed
  • Same as of H – vrms speed
  • half of H – vrms speed
At temperature T, the rms speed of helium molecules is the same as rms speed of hydrogen molecules at normal temperature and pressure. The value of T is
  • 546o C
  • 0o C
  • 273o C
  • 136.5o C
The root mean square speed of hydrogen molecules at 300 K is 1930 m/s. Then the root mean square speed of Oxygen molecules at 900 K will be
  • 836 m/s
  • 643 m/s

  • Physics-Kinetic Theory of Gases-75372.png

  • Physics-Kinetic Theory of Gases-75373.png
If rms speed of a gas is vrms = 1840 m/s and its density ρ = 8.99 × 10–2 kg/m3 , the pressure of the gas will be

  • Physics-Kinetic Theory of Gases-75375.png
  • 2)
    Physics-Kinetic Theory of Gases-75376.png

  • Physics-Kinetic Theory of Gases-75377.png

  • Physics-Kinetic Theory of Gases-75378.png
The rms speed of a gas at a certain temperature is √2 times than that of the Oxygen molecule at that temperature, the gas is_____
  • SO2
  • CH4
  • H2
  • He
A monoatomic gas molecule has
  • Three degrees of freedom
  • Five degrees of freedom
  • Six degrees of freedom
  • Four degrees of freedom
A diatomic molecule has how many degrees of freedom (For rigid rotator)
  • 4
  • 3
  • 6
  • 5

Physics-Kinetic Theory of Gases-75381.png

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  • 2)
    Physics-Kinetic Theory of Gases-75383.png

  • Physics-Kinetic Theory of Gases-75384.png

  • Physics-Kinetic Theory of Gases-75385.png
A diatomic gas molecule has translational, rotational and vibrational degrees of freedom. The Cp/Cv is
  • 1.29
  • 1.33
  • 1.4
  • 1.67
The value of Cv for one mole of neon gas is

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    Physics-Kinetic Theory of Gases-75389.png

  • Physics-Kinetic Theory of Gases-75390.png

  • Physics-Kinetic Theory of Gases-75391.png
The relation between two specific heats of a gas is

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    Physics-Kinetic Theory of Gases-75394.png

  • Physics-Kinetic Theory of Gases-75395.png

  • Physics-Kinetic Theory of Gases-75396.png
The figure shows the volume V versus temperature T graphs for a certain mass of a perfect gas at two constant pressure of P1 and P2. What inference can you draw from the graphs.
Physics-Kinetic Theory of Gases-75403.png
  • P1 < P2
  • P1 > P2
  • P1 = P2
  • No inference can be drawn due to insufficient information
Which one the following graphs represents the behaviour of an ideal gas

  • Physics-Kinetic Theory of Gases-75405.png
  • 2)
    Physics-Kinetic Theory of Gases-75406.png

  • Physics-Kinetic Theory of Gases-75407.png

  • Physics-Kinetic Theory of Gases-75408.png
Under constant temperature, graph between p and 1/V is
  • Hyperbola
  • Circle
  • Parabola
  • Straight line
Assertion : The time of collision of molecules is of the order of 10–8 s, which is very very small compared to the time between two successive collisions.
Reason : This is an experimental fact.
  • If both Assertion and Reason are true and the Reason is correct explanation of the Assertion
  • If both Assertion and Reason are true, but Reason is not correct explanation of the Assertion
  • If Assertion is true; the Reason is false
  • If Assertion is false, but the reason is true
The temperature of a gas at pressure P and volume V is 27°C. Keeping the volume constant if its temperature is raised to 927C, then its pressure will he
  • 2 P
  • 3 P
  • 4 P
  • 6 P
When a van der waal’s gas undergoes free expansion then its temperature
  • Decreases
  • Increases
  • Does not change
  • Depends upon the nature of the gas
Volume, pressure and temperature of an ideal gas are V, P and T respectively. If mass of its molecules is m, then its density is [k= boltzmann’s constant)

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    Physics-Kinetic Theory of Gases-75412.png

  • Physics-Kinetic Theory of Gases-75413.png

  • Physics-Kinetic Theory of Gases-75414.png
Boyle’s law holds for an ideal gas during
  • Isobaric changes
  • Isothermal changes
  • Isochoric changes
  • Isotonic changes
S.I. unit of universal gas constant is
  • cal/°C
  • J/mol
  • J mol–1 K–1
  • J/kg
Molecules of a gas behave like
  • Inelastic rigid sphere
  • Perfectly elastic non-rigid sphere
  • Perfectly elastic rigid sphere
  • Inelastic non-rigid sphere
The volume of a gas at 20°C is 200 ml. If the temperature is reduced to –20°C at constant pressure, its volume will be
  • 172.6 ml
  • 17.26 ml
  • 192.7 ml
  • 19.27 ml

Physics-Kinetic Theory of Gases-75417.png
  • 0.32
  • 0.45
  • 2.24
  • 3.16
The vapour of a substance behaves as a gas
  • Below critical temperature
  • Above critical temperature
  • At 100°C
  • At 1000°C
If the volume of the gas containing n number of molecules is V, then the pressure will decrease due to force of intermolecular attraction in the proportion

  • Physics-Kinetic Theory of Gases-75419.png
  • 2)
    Physics-Kinetic Theory of Gases-75420.png

  • Physics-Kinetic Theory of Gases-75421.png

  • Physics-Kinetic Theory of Gases-75422.png
What is the mass of 22.4 atmospheric pressure 2 litres of nitrogen at and 273 K
  • 28 g
  • 56 g
  • 4 × 22.4 g
  • None of these
Which of the following statements about kinetic theory of gases is wrong?
  • The molecules of a gas are in continuous random motion
  • The molecules continuously undergo inelastic collisions
  • The molecules do not interact with each other except during collisions
  • The collisions amongst the molecules are of short duration
A person blows into open-end of a long pipe. As a result, a high-pressure pulse of air travels down the pipe. When this pulse reaches the other end of the pipe,
  • a high-pressure pulse starts travelling up the pipe, if the other end of the pipe is open
  • a low-pressure pulse starts travelling up the pipe, if the other end of the pipe is open
  • a low-pressure pulse starts travelling up the pipe, if the other end of the pipe is closed
  • a high-pressure pulse starts travelling up the pipe, if the other end of the pipe is closed
0:0:1


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