JEE Questions for Chemistry States Of Matter Quiz 2 - MCQExams.com

The ratio of the rate of diffusion of helium and methane under identical condition of pressure and temperature will be
  • 4
  • 0.2
  • 2
  • 0.5
Graham's law deals with the relation between
  • pressure and volume
  • density and rate of diffusion
  • rate of diffusion and volume
  • rate of diffusion and viscosity
Which gas has the highest partial pressure atmosphere?
  • CO2
  • H2 O
  • O2
  • N2
If the temperature of 500 mL of air increases from 27°C to 42°C under constant pressure, then the increases in volume shall be
  • 15 mL
  • 20 mL
  • 25 mL
  • 30 mL
For an ideal gas, number of mol per litre in terms of its pressure p, temperature T and gas constant R is
  • pT / R
  • pRT
  • p / RT
  • RT / p
At what temperature will the rms velocity of SO2 be the same as that of O2 at 303 K?
  • 403 K
  • 303 K
  • 606 K
  • 273 K
The molecular velocity of any gas is
  • inversely proportional to the square root of temperature
  • inversely proportional to absolute temperature
  • directly proportional to square of temperature
  • directly proportional to square root of temperature
The root mean square velocity of a gas is doubled when temperature is
  • increased four times
  • increased two times
  • reduced to half
  • reduced to one-fourth
Different gases at the same temperature have same
  • pressure
  • number of moles
  • volume
  • average kinetic energy
The rms velocity of an ideal gas at constant pressure varies with density (d) as

  • Chemistry-States of Matter-7547.png
  • d

  • Chemistry-States of Matter-7548.png
  • d2
At the same temperature, calculate the ratio of average velocity of SO2 to CH4 .
  • 2 : 3
  • 3 : 4
  • 1 : 2
  • 1 : 6
Kinetic energy of one mole of an ideal gas at 300 K (in kJ) is
  • 3.74
  • 348
  • 34.8
  • 3.48
Ratio of average to most probable velocity is
  • 1.128
  • 1.224
  • 1.0
  • 1.112
Equal masses of H2,O2 and methane have been taken in a container of volume V at temperature 27°C in identical conditions. The ratio of the volumes of gases H2 : O2 : methane would be :
  • 8 : 16 : 1
  • 16 : 8 : 1
  • 16 : 1 : 2
  • 8 : 1 : 2
Vapour pressure increases with increase in
  • concentration of solution containing non-volatile solute
  • temperature upto boiling point
  • temperature upto triple point
  • altitude of the concerned place of boiling
The following is a method to determine the surface tension of liquids
  • single capillary method
  • refractometric method
  • polarimetric method
  • boiling point method
Which of the following set of variables give a straight line with a negative slope when plotted?
(p = vapour pressure, T = temperature in K)
  • Y-axis = p , X-axis = T
  • Y-axis = log10 p , X-axis = T
  • Y-axis = log10 p , X-axis = 1/T
  • Y-axis = log10 p , X-axis = log10 1/T
If Z is a compressibility factor, van der Waals' equation at low pressure can be written as

  • Chemistry-States of Matter-7550.png
  • 2)
    Chemistry-States of Matter-7551.png

  • Chemistry-States of Matter-7552.png

  • Chemistry-States of Matter-7553.png
Find the pressure of a sample of CCl4 , if 1.0 mole occupies 35 L at 77°C. Assume CCl4 obeys the van der Waals equation of state. (a = 20 L2 mol-2 atm and b = 0.14 L mol-2)
  • 0.56 atm
  • 0.572 atm
  • 0.82 atm
  • 0.807 atm
The compressibility factor (Z) of one mole of a van der Waals' gas of negligible 'a ' value is
  • 1
  • 2)
    Chemistry-States of Matter-7554.png

  • Chemistry-States of Matter-7555.png

  • Chemistry-States of Matter-7556.png
50 mL of each gas A and of gas B takes 150 and 200 seconds respectively for effusing through a pin hole under the similar condition. If molecular mass of gas B is 36, the molecular mass of gas A will be :
  • 96
  • 128
  • 32
  • 64
  • None of the above
For one mole of a van der Waals' gas when b = 0 and T = 300 K, the pV versus 1/V plot is shown below. The value of the van der Waals' constant a (atm L mol-2 ) is
Chemistry-States of Matter-7559.png
  • 1.0
  • 4.5
  • 1.5
  • 3.0
a and b are van der Waals' constants for gases. Chlorine is more easily liquefied than ethane because
  • a and b for Cl2 > a and b for C2 H6
  • a and b for Cl2 < a and b for C2 H6
  • a for Cl2 > a for C2 H6 but b for Cl2 > b for C2 H6
  • a for Cl2 > a for C2 H6 but b for Cl2 < b for C2 H6
Pressure exerted by 1 mole of methane in a 0.25 L container at 300 K using van der Waals' equation is
(given, a = 2.253 atm L2 mol-2 , b= 0.0428 L mol-1 )
  • 82.82 atm
  • 152.51 atm
  • 190.52 atm
  • 70.52 atm
When a sample of gas is compressed at constant temperature from 15 atm to 6 atm, its volume changes from 76 cm3 to 20.5 cm3. Which of the following statements are possible explanations of this behaviour?
I. The gas behaves non-ideally.
II. The gas dimerises.
III. The gas is absorbed into the vessel walls.
  • I, II and III
  • I and II only
  • II and III
  • Only I
  • Only III
The temperature, at which a gas shows maximum ideal behaviour, is known as
  • Boyle's temperature
  • inversion temperature
  • critical temperature
  • absolute temperature
The units of van der Waals' constants a, b respectively, are
  • L atm2 mol-1 and mol L-1
  • L atm mol2 and mol L-1
  • L2 atm mol-2 and mol -1 L
  • L-2 atm-1 mol-1 and L mol -2
The CO2 gas does not follow gaseous laws at all ranges of pressure and temperature because
  • it is triatomic gas
  • its internal energy is quite high
  • there is attraction between its molecules
  • it solidify at low temperature
Which one, among the following, is the van der Waals' equation, describing the behaviour of one mole of a real gas over wide ranges of temperature and pressure?

  • Chemistry-States of Matter-7560.png
  • 2)
    Chemistry-States of Matter-7561.png

  • Chemistry-States of Matter-7562.png

  • Chemistry-States of Matter-7563.png
A gaseous mixture containing He, CH4 and SO2 was allowed to effuse through a fine hole, then find what molar ratio of gases coming out initially? (Given mixture contains He, CH4 and SO2 in 1 : 2 : 3 mole ratio).

  • Chemistry-States of Matter-7564.png
  • 2 : 2 : 3
  • 4 : 4 : 3
  • 1 : 1 : 3
0:0:1


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