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LEARNERS HABITAT
1] A spherical balloon of 21 cm diameter and 4.851 L volume is to be filled with hydrogen
at NTP from a cylinder containing the gas at 20 atm and 27
0
C. The cylinder can hold
2.82 L of water at NTP. What will be the number of balloons that can be filled up?
a) 5 b) 10 c) 15 d) 20
2] An L. P. G. cylinder contains 15 kg of butane gas at 27
0
C and 10 atmospheric pressure. It
was leaking and its pressure fell down to 8 atmospheric pressure after one day. The gas
leaked in 5 days is
a) 10 kg b) 3 kg c) 15 kg d) 12 kg
3] A flask containing air (open to the atmosphere) is heated from 300 K to 500 K. then % of
air escaped to the atmosphere is 
a) 20.0 b) 40 c) 60 d) 80
4] For X g of ideal gas V and V 0 are the volumes at t
0
C and 0
0
C respectively at 1 atm
pressure so that V/V0 = (1 + ? t). Here, ? is
a) < 1 b) < 0 c) > 1 d) = 0
5] The values of critical temperatures (Tc) and critical pressure (Pc) for some gases are
given below. Which of the gases cannot be liquefied at 100 K and 50 atm?
Gases A B C D 
P c(atm) 2.2 14 35 45 
Tc(K) 5.1 33 127 140 
a) D only b) A only c) A and b d) C and D
6] The compressibility of gas < unity at STP. Therefore
a) V m = 22.4 L b) V m < 22.4 L c) V m = 22.4 L d) V m = 44.8 L
7] Open end manometer was connected to gas chamber. The Hg level stood 15 mm higher
in the open end as compared to the end connected to gas chamber. If the atmospheric
pressure is 101.3 kPa. The gas pressure in kPa is
a) 103.3 b) 101.3 c) 94.3 d) 115.3
8] What is wrong about the 50 L vessel that contains dioxygen and dihydrogen in the 
molar ratio of 1:1, at a pressure 101.3 kPa?
a) H2 molecules move faster than oxygen
b) Each gas has same number of molecules
c) If O2 is removed from the mixture, the pressure will fall to 25.3 kPa
d) On the average, the molecular impacts of H 2 on the walls per unit time are larger than 
those of oxygen
9] 5.0 dm
3
 of water is placed in a closed room of volumes 2.5 x 10
4
 dm3 at 300 k if vapour 
pressure of water is 0.036 bars and its density is 0.990 g cm
-3
, the volume of water left in 
liquid state is 
a) 4.34 dm
3
b) 3.44 dm
3
c) 2.5dm
3
d) 4.5 dm
3 
LH Practice Sheet GASEOUS STATE
LEARNERS HABITAT, 97/1, 3rd Floor, Near NCERT Gate No. 01, Adchini, New Delhi. +91-8510800081/82 
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FAQs on Gaseous State (Advanced) - Practice Sheet, Class 11, Chemistry - JEE

1. What is the definition of the gaseous state in chemistry?
Ans. The gaseous state in chemistry refers to the physical state of matter in which substances exist as gases. Gases have no definite shape or volume and can expand to fill the container they are placed in. They are composed of particles that are far apart and move freely in all directions.
2. How is the behavior of gases described in the gaseous state?
Ans. The behavior of gases in the gaseous state is described using the kinetic molecular theory. According to this theory, gases are composed of particles (atoms, molecules, or ions) that are in constant random motion. The motion of these particles is influenced by factors such as temperature, pressure, and volume.
3. What are the main properties of gases in the gaseous state?
Ans. The main properties of gases in the gaseous state include: 1. Compressibility: Gases can be easily compressed due to the large spaces between their particles. 2. Expandability: Gases can expand to fill the container they are placed in. 3. Fluidity: Gases flow easily and have no definite shape. 4. Low density: Gases have low densities compared to solids and liquids. 5. Diffusibility: Gases mix and spread out rapidly when in contact with each other.
4. How does the pressure of a gas change with temperature in the gaseous state?
Ans. According to Charles's law, the pressure of a gas is directly proportional to its temperature, provided that the volume and amount of gas remain constant. This means that as the temperature of a gas increases, its pressure also increases, and vice versa. The relationship between pressure and temperature is expressed by the equation P1/T1 = P2/T2, where P1 and T1 represent the initial pressure and temperature, and P2 and T2 represent the final pressure and temperature.
5. How do real gases differ from ideal gases in the gaseous state?
Ans. Real gases differ from ideal gases in the gaseous state due to the presence of intermolecular forces and the finite size of gas particles. Ideal gases are assumed to have no intermolecular forces and occupy no volume, while real gases do experience intermolecular forces and occupy a certain volume. These factors can cause deviations from ideal gas behavior, especially at high pressures and low temperatures. Real gases follow the ideal gas laws more closely under conditions of low pressure and high temperature.
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