Gaseous State Test

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Gaseous State Test - 11

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Weekly Quiz Competition

Question 1
4 / -1

The ratio of root mean square velocity to average velocity of a gas molecule at a particular temperature is:

A
1.086 : 1

B
1 : 1.086

C
2 : 1.086

D
1.086 : 2

Solution
Question 2
4 / -1

The temperature at which a real gas obeys the ideal gas laws over a wide range of pressure is:

A
Critical temperature

B
Boyle temperature

C
Inversion temperature

D
Reduced temperature
Solution
The temperature at which the real or non-ideal gas behaves as an ideal gas over a wide range of pressure is known as Boyle temperature.
Boyle temperature (T_B) is related to the Vander Waal’s constant a, b as given below. At this temperature, the attractive and repulsive forces acting on the gas particles arrive at a balance for a real gas.
T_B= a/Rb
Question 3
4 / -1

Equal weights of methane and oxygen and mixed in an empty container at 25°C. The fraction of the total pressure exerted by oxygen is:

A
1/3

B
1/2

C
2/3

D
(1/3) × (273/298)

Solution

Let the mass of methane and oxygen be m gm.
Mole fraction of oxygen, x_O2 = m/32/(m/32 +m/16) = 1/3
Let the total pressure be P.
Partial pressure of O₂, p_O2 = P × x_O2 = P x 1/3 = P/3
Question 4
4 / -1

Helium atom is two times heavier than a hydrogen molecule. At 298 K, the average kinetic energy of a helium atom is:

A
Two times that of a hydrogen molecule

B
Same as that of a hydrogen molecule

C
Four times that of a hydrogen molecule

D
Half that of a hydrogen molecule

Solution

Kinetic energy of gas molecule depends on temperature and does not depend upon the nature of gas.
K.E =(3/2)kT.
Thus hydrogen and helium have same K.E at same temperature
Question 5
4 / -1

No cooling occurs, when an ideal gas undergoes unrestrained expansion, because the molecules:

A
collide without loss of energy.

B
do work equal to loss in kinetic energy.

C
are above the inversion temperature.

D
exert no attractive force on each other.

Solution

Ideal gas has no attractive force between the particles
Question 6
4 / -1

A liquid is in equilibrium with its vapour at it’s boiling point. On the average, the molecules in the two phases have equal:

A
Inter-molecular forces

B
Potential energy

C
Kinetic energy

D
Total energy

Solution

When a liquid is in equilibrium with its vapout at its boiling point, the molecules in the two phases have equal kinetic energy.
At equilibrium, the rate of molecules going from the liquid to the gaseous phase equal to the rate of molecules going from the gaseous phase to the liquid surface and hence they have equal kinetic energy.
Question 7
4 / -1

Rate of diffusion of a gas is:

A
Directly proportional to its density

B
Directly proportional to its molecular weight

C
Directly proportional to the square root of its molecular weight.

D
Inversely proportional to the square root of its molecular weight.

Solution

Graham's law states that the rate of diffusion or of effusion of a gas is inversely proportional to the square root of its molecular weight.
Rate of Diffusion is proportional to 1/ √M
Question 8
4 / -1

The average velocity of an ideal gas molecule at 27°C is 0.3 m/s. The average velocity at 927°C will be

A
0.6 m/s

B
0.3 m/s

C
0.9 m/s

D
3.0 m/s

Solution
Question 9
4 / -1

In van der Waals’ equation of state for a non-ideal gas, the term that accounts for intermolecular forces is:

A
(V – b)

B
RT

C

D
(RT)^–1

Solution

In van der Waals’ equation of state:
(p + a/V²) (V - b) = RT (for 1 mole)
The first factor (p + a/V₂) correct for intermolecular force while the second term (V - b) correct for molecular volume.
Question 10
4 / -1

A bottle of dry ammonia and a bottle of dry hydrogen chloride connected through a long tube are opened simultaneously at both ends the white ammonium chloride ring first formed will be:

A
At the centre of the tube

B
Near the hydrogen chloride bottle

C
Near the ammonia bottle

D
Throughout the length of the tube.
Solution
According to Graham's law of effusion:
Rate of effusion = √(1/Molar mass)
i.e. Gas of higher molar mass will effuse slowly, therefore, move a shorter distance.
NH₃ molar mass is 17 and HCl molar mass is 36.5. So, HCl effuses slowly and the formation of NH₄Cl white rings are formed near the HCl

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Gaseous State Test - 11

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Gaseous State Test - 11

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Question 1

1.086 : 1

1 : 1.086

2 : 1.086

1.086 : 2

Solution

Question 2

Critical temperature

Boyle temperature

Inversion temperature

Reduced temperature

Solution

Question 3

1/3

1/2

2/3

(1/3) × (273/298)

Solution

Question 4

Two times that of a hydrogen molecule

Same as that of a hydrogen molecule

Four times that of a hydrogen molecule

Half that of a hydrogen molecule

Solution

Question 5

collide without loss of energy.

do work equal to loss in kinetic energy.

are above the inversion temperature.

exert no attractive force on each other.

Solution

Question 6

Inter-molecular forces

Potential energy

Kinetic energy

Total energy

Solution

Question 7

Directly proportional to its density

Directly proportional to its molecular weight

Directly proportional to the square root of its molecular weight.

Inversely proportional to the square root of its molecular weight.

Solution

Question 8

0.6 m/s

0.3 m/s

0.9 m/s

3.0 m/s

Solution

Question 9

(V – b)

RT

(RT)–1

Solution

Question 10

At the centre of the tube

Near the hydrogen chloride bottle

Near the ammonia bottle

Throughout the length of the tube.

Solution

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(RT)^–1