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A gas at 350K and 15 bar has molar volume 20 percent smaller than that for an ideal gas under the same conditions. The  correct  option about the gas and its compressibility factor (Z) is:

• Option 1)

Z>1 and attractive forces are dominant

• Option 2)

Z>1 and repulsive forces are dominant

• Option 3)

Z<1 and attractive forces are dominant

• Option 4)

Z<1 and repulsive forces are dominant

Option 3          Molar volume of gas is 20% smaller than that of the ideal gas. Hence Z < 1 and attractive forces are dominant. When Z < 1: Gas shows negative deviation and is more compressible than expected from ideal behaviour.  Z < 1 corresponds to attractive forces between molecules.Option 1)Z>1 and attractive forces are dominantOption 2)Z>1 and repulsive forces are dominantOption 3)Z<1...
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A gas is allowed to expand at constant temperature from a volume of 400 ml to a volume of one litre. The final pressure of gas is 100mm of Hg. The initial pressure of the gas in nm is 1) 100 2) 200 3) 2504) 500
PV=constant P1V1=P2V2 P1*400=100*1000 P1= 250 option 3) is correct.
Medical
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The van't Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is

• Option 1)

0

• Option 2)

1

• Option 3)

2

• Option 4)

3

As we learned in concept Clearly van't Hoff factor is 3 Option 1) 0 This option is incorrect. Option 2) 1 This option is incorrect. Option 3) 2 This option is incorrect. Option 4) 3 This option is correct.
Medical
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The correction factor 'a' to the ideal gas equation corresponds to

• Option 1)

electric held present between the gas molecules

• Option 2)

volume of the gas molecules

• Option 3)

density of the gas molecules

• Option 4)

forces of attraction between the gas molecules

As we learnt that Vander waal constants - Vander waal constant ‘a’ is measure of intermolecular attraction of a gas -    Vanderwaal constant (a)   force of attraction   Option 1) electric held present between the gas molecules This is incorrect. Option 2) volume of the gas molecules This is incorrect. Option 3) density of the gas molecules This is incorrect. Option 4)  forces of attraction...
Medical
419 Views   |

Given van der Waals constant for NH3, H2, O2 and CO2 are respectively 4.17, 0.244, 1.36 and 3.59, which one of the following is most easily liquefied ?

• Option 1)

O2

• Option 2)

H2

• Option 3)

NH3

• Option 4)

CO2

As we learnt that Liquefaction of gases - converting real gas into liquid state at high pressure and low temperature -    Ease of liquifcation of gas depends on intermolecular interaction between gas molecule. NH3 has dipole - dipole interaction so it can easily liquify.   Option 1) O2 This is incorrect. Option 2) H2 This is incorrect. Option 3) NH3 This is correct. Option 4) CO2 This is incorrect.
Medical
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A gaseous mixture was prepared by taking equal mole of $CO_{2}\ and\ N_{2}$ . If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen $\left ( N_{2} \right )$ in the mixture is:

• Option 1)

0.5 atm

• Option 2)

0.8 atm

• Option 3)

0.9 atm

• Option 4)

1 atm

Partial Pressure of a gas in gaseous mixture - Partial Pressure = (Total Pressure of Mixture)  (mole fraction of gas)   -     Option 1) 0.5 atm This solution is correct  Option 2) 0.8 atm This solution is incorrect  Option 3) 0.9 atm This solution is incorrect  Option 4) 1 atm This solution is incorrect
Medical
117 Views   |

A gas such as carbon monoxide would be most likely to obey the ideal gas law at:

• Option 1)

High temperatures and low pressure.

• Option 2)

Low temperatures and high pressure.

• Option 3)

High temperatures and high pressure.

• Option 4)

Low temperatures and low pressure.

Ideal Gas Law - - wherein P - Pressure V - Volume n - No. of Moles R - Gas Constant T - Temperature    A real gas can behave as an ideal gas if volume of molecule is negligible and interaction between the molecule is negligible. This will happen when number of molecule per unit volume is very small.  From ideal gas equation,  will be very large if  is very large and  is very...
Medical
111 Views   |

A bubble of air is underwater at temperature $15^{o}C$ and the pressure 1.5bar. If the bubble rises to the surface where the temperature is $25^{o}C$ and the pressure is 1.0 bar, What will happen to the volume of the bubble?

• Option 1)

Volume will become greater by a factor of 1.6

• Option 2)

Volume will become greater by a factor of 1.1

• Option 3)

Volume will become smaller by a factor of 0.70

• Option 4)

Volume will become greater by a factor of 2.5

Ideal Gas Law - - wherein P - Pressure V - Volume n - No. of Moles R - Gas Constant T - Temperature    We know that from ideal gas equation given K= 288K, = 293 K, Option 1) Volume will become greater by a factor of 1.6 This is correct answer Option 2) Volume will become greater by a factor of 1.1 This is incorrect answer Option 3) Volume will become smaller by a factor of...
Medical
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Two gases A and B having the same volume diffuse through a porous partition in 20 and 10 second respectively. The molecular mass of A is 49u. Molecular mass of B will be

• Option 1)

50.00u

• Option 2)

12.25u

• Option 3)

6.50u

• Option 4)

25.00u

Graham’s law of diffusion -   where r is rate of diffusion of gas , M is molar mass. -    As we know => Option 1) 50.00u This is incorrect answer Option 2) 12.25u This is correct answer Option 3) 6.50u This is incorrect answer Option 4) 25.00u This is incorrect answer
Medical
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Equal moles of hydrogen and oxygen gases are placed in a container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the hydrogen to escape?

• Option 1)

1/8

• Option 2)

1/4

• Option 3)

3/8

• Option 4)

1/2

As we learnt in Graham’s law of diffusion -   where r is rate of diffusion of gas , M is molar mass. -    Let the number of moles of each gas =x Fraction of hydrogen escaped = Hence fraction of oxygen escaped =   Option 1) 1/8 This is correct answer Option 2) 1/4 This is incorrect answer Option 3) 3/8 This is incorrect answer Option 4) 1/2 This is incorrect answer
Medical
771 Views   |

Equal masses of H2, O2 and methane have been taken in a container of volume V at temperature 27oC in identical conditions. The ratio of the volumes of gases H2:O2: methane would be :

• Option 1)

8 : 16 : 1

• Option 2)

16 : 8 : 1

• Option 3)

16: 1 : 2

• Option 4)

8 : 1 : 2

As learnt in Partial Pressure of a gas in gaseous mixture - Partial Pressure = (Total Pressure of Mixture)  (mole fraction of gas)   -     Suppose mass is m moles of  = m/2 moles of  = m/32 moles of methane = m/16 Volume ratio =  = 16:1:2 Option 1) 8 : 16 : 1 This solution is incorrect. Option 2) 16 : 8 : 1 This solution is incorrect. Option 3) 16: 1 : 2 This solution is correct. Option 4) 8...
Medical
589 Views   |

A mixture of gases contains H2 and O2 gases in the ratio of 1 : 4 (w/w). What is the molar ratio of the two gases in the mixture ?

• Option 1)

16 : 1

• Option 2)

2 : 1

• Option 3)

1 : 4

• Option 4)

4 : 1

Partial Pressure of a gas in gaseous mixture - Partial Pressure = (Total Pressure of Mixture)  (mole fraction of gas)   -    suppose mass of     = then, mass of   =  Moles of   Moles of      Option 1) 16 : 1 This option is incorrect. Option 2) 2 : 1 This option is incorrect. Option 3) 1 : 4 This option is incorrect. Option 4) 4 : 1 This option is correct.
Medical
1537 Views   |

Equal moles of hydrogen and oxygen gases are placed in a container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the hydrogen to escape?

• Option 1)

1/8

• Option 2)

1/4

• Option 3)

3/8

• Option 4)

1/2

As we learned in concept Graham’s law of diffusion -   where r is rate of diffusion of gas , M is molar mass. -    By  graham's law of diffusion of gas Option 1) 1/8 Option is correct Option 2) 1/4 Option is incorrect Option 3) 3/8 Option is incorrect Option 4) 1/2 Option is incorrect
Medical
248 Views   |

A gas such as carbon monoxide would be most likely to obey the ideal gas law at:

• Option 1)

high temperatures and low pressures.

• Option 2)

low temperatures and high pressures.

• Option 3)

high temperatures and high pressures.

• Option 4)

low temperatures and low pressures.

As we learned in concept no Kinetic Theory of Gases - Molecules of gases are very small and their actual volume is negligible in comparision to the empty space between them. -    Ideal gas behaviour is based on the following assumption molecules of gases are very small and their actual volume is negligible in comparision to the empty space between them There is no force of attraction between...
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