According to kinetic theory of gases, for a diatomic molecule

(A) The pressure exerted by the gas is proportional to the mean velocity of the molecule.

(B) The pressure exerted by the gas is proportional to the root mean square velocity of the molecule.

(C) The root mean square velocity of the molecule is inversely proportional to the temperature.

(D) The mean translational kinetic energy of the molecule is proportional to the absolute temperature.

Concept Questions :-

Kinetic Theory of Gas
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The values of vander waals constant ‘a’ for the gases O2, N2NH3 and CH4 are 1.36, 1.39, 4.17 and 2.253 lit2 atom mol-2 respectively. The gas which can most easily be liquefied is-

(A) O2                                 

(B) N2

(C) NH3                              

(D) CH4

Concept Questions :-

Vanderwaal Correction
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At low pressure, the vander waals equation is written as :

(A) Z=1-aRTV                                 

(B) Z=1-RTVa

(C) Z=1+aRTV                                 

(D) Z=1+RTVa

Concept Questions :-

Vanderwaal Correction
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X ml of H2 gas effuses through a hole in a container in 5 seconds. The time taken for the effusion of the same volume of the gas specified below under ideal condition is

(A) 10 seconds : He                          

(B) 20 seconds : O2

(C) 25 seconds : CO                          

(D) 55 seconds : CO2

Concept Questions :-

Graham's Law
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The valves X and Y are opened simultaneously. The white fumes of NH4Cl will first form at :

  

(A) A                                                 

(B) B

(C) C                                                 

(D) A, B and C simultaneously

Concept Questions :-

Graham's Law
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A gas mixture consists of 2 moles of oxygen and 4 moles of a argon at temperature T. Neglecting all vibrational modes, the total internal energy of the system is –

(A) 4RT                         

(B) 5RT

(C) 15RT                       

(D) 11RT

Concept Questions :-

Kinetic Theory of Gas
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Given reaction : Cs + H2Og  COg + H2g. Calculate the volume at STP from 48 gm of carbon and excess H2O-

(A) 179.2 lit.                           

(B) 89.6 lit.

(C) 44.8 lit.                             

(D) 22.4 lit.

Concept Questions :-

Ideal Gas Law
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Two gases occupy two containers A and B the gas in A, of volume 0.10 m3, exerts a pressure of 1.40 MPa and that in B of volume 0.15 m3 exerts a pressure 0.7 MPa. The two containers are united by a tube of negligible volume and the gases are allowed to intermingle. Then if the temperature remains constant, the final pressure in the container will be (in MPa)

(A) 0.70                               

(B) 0.98

(C) 1.40                               

(D) 210

Concept Questions :-

Ideal Gas Law
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The average molecular weight of air is 28.8 g mol1. At 20ºC, the pressure of air at a height of 6 km is half of that at the sea level. Assuming that air contains minute quantities of hydrogen, at what height the partial pressure of hydrogen would be one fourth of the partial pressure at the sea level ? The temperature may be assumed to be the same.

(A) 172.8 km                           

(B) 4.8 km

(C) 86.4 km                             

(D) 9.6 km

Concept Questions :-

Ideal Gas Law
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2.3 grams of a mixture of NO2 and N2O4 have a pressure of 0.82 atm at temperature, T K and volume, V litres. If VT=1300magnitude, calculate PNO2. Assume that all the NO2 was formed N2O4.

(A) 0.52 atm                             

(B) 0.38 atm

(C) 0.19 atm                             

(D) 0.41 atm

Concept Questions :-

Dalton's Law
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