Gaseous States Test

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Gaseous States Test - 10

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Weekly Quiz Competition

Question 1
1 / -0

If the four tubes of a car are filled to the same pressure with N₂, O₂, H₂ and Ne separately, then which one will be filled first?

A
N₂

B
O₂

C
Ne

D
H₂

Solution

Given gases are N₂, O₂ ,H₂ and Ne.

Molecular weight N₂ = 28gm

O₂= 16gm

H₂= 2gm

Ne = 20.2gm

∴ Diffusion Rate of H₂ is mole. So, H₂ will be filled first.
Question 2
1 / -0

Use of hot air balloons in sports and for meteorological observations is an application of

A
Boyle’s law

B
Newton’s law

C
Kelvin’s law

D
Charle’s law

Solution

The Charles’s law is the use of hot air balloons in sports and for meteorological observations gas expands on heating. Since the mass of gas sample is constant, the larger volume at higher temperature will have lower mass per unit volume and therefore lower density. Thus hot air is less dense than cold air. This causes a hot air balloon to rise by displacing cool air of the atmosphere.
Question 3
1 / -0

Kinetic theory of gases presumes the collision between the molecules to be perfectly elastic because:

A
the molecules are rigid

B
the temperature remains constant irrespective of collisions

C
collisions will not split the molecules

D
the molecules are tiny

Solution

The kinetic theory of gases presumes the collision between the molecules to be perfectly elastic because the molecules are tiny. If the molecules are tiny, the energy and momenta of the molecules are conserved during the collisions. Consequently, the temperature remains constant irrespective of collisions.
Question 4
1 / -0

Air at sea level is dense. This is a practical application of

A
Boyle's law

B
Charle's law

C
Avogadro's law

D
Dalton's law

Solution

At sea level, because of compression by air above the proximal layer of air, pressure increases hence volume decreases i.e. density increases. It is Boyle's law.
Question 5
1 / -0

The temperature of a gas is raised from 27^oC to 927^oC. The root mean square speed

A
Gets halved

B
Gets doubled

C

D
Remains the same

Solution

Given, T₁= 27^oC = 300K

T₂= 927^oC = 1200K
Question 6
1 / -0

If 20 L of a gas at 1 atm is expanded to 50 L at constant T, then what is the final pressure?

A
20 × 1/50

B
50 × 1/20

C
1 × 1/20 × 50

D
None of these

Solution

From ideal gas equation,

PV = nRT

For same no. of moles of a gas at constant temperature,

PV = Constant

Hence the final pressure will be 20 × 1/50.
Question 7
1 / -0

When the temperature of 23ml of dry CO₂ gas is changed from 10^∘ to 30^∘ at constant pressure of 760 mm, the volume of gas becomes closest to which one of the following?

A
7.7 ml

B
21.5 ml

C
24.6 ml

D
69 ml

Solution

According to charles Law,
Question 8
1 / -0

The pressure of 2 moles of ideal gas at 546K having volume 44.8L is:

A
2 atm

B
3 atm

C
4 atm

D
1 atm

Solution

PV = nRT

Given n = 2, T = 546K, V = 44.8L
Question 9
1 / -0

Equal volumes of two gases which do not react together are enclosed in separate vessels. Their pressure are 100mm and 400 mm respectively. If the two vessels are joined together, then what will be the pressure of the resulting mixture ( temperature remaining constant )

A
125 mm

B
500 mm

C
1000 mm

D
250 mm

Solution

When two vessels are joined together, volume will be doubled hence effective pressure will be halved.
Question 10
1 / -0

An open flask containing air is heated from 300 K to 500 K . What percentage of air will be escaped to the atmosphere, if pressure is kept constant?

A
80

B
40

C
60

D
20

Solution