CBSE Questions for Class 11 Medical Chemistry States Of Matter Gases And Liquids Quiz 2 - MCQExams.com

Which of the following mixture does not obey Dalton's law of partial pressures?
  • $$SO_{2}+Cl_{2}$$
  • $$NH_{3}+PH_{3}$$
  • $$CO_{2}+N_{2}$$
  • $$CO+CO_{2}$$
An ideal gas is one which obeys?
  • Boyle's law
  • Gas laws
  • Charle's law
  • Avogadro law
Kinetic energy of molecules is highest in:
  • gases
  • solids
  • liquids
  • solutions
Which of the following is a representation of Gay-Lussac's law?          
  • $$P_{1}T_{1}=P_{2}T_{2}$$
  • $$P_{1}T_{2}=P_{2}T_{1}$$
  • $$P_{1}V_{1}=P_{2}V_{2}$$
  • $$V_{1}T_{2}=V_{2}T_{1}$$
Which has maximum value of mean free path?
  • $$CO_{2}$$
  • $$H_{2}$$
  • $$O_{2}$$
  • $$N_{2}$$
The pressure of a gas is due to:
  • the collision of gas molecules against each other
  • the random movement of gas molecules
  • the intermolecular forces of attraction between the gas molecules
  • the collision of gas molecules against the walls of the container
Gram molar volume for a gas is always considered at ___ conditions.
  • NTP
  • STP
  • variable temperature
  • none of these
Volume of gas at STP is $$1.12\times 10^{-7}cc$$. Calculate the number of a molecule in it.
  • $$3.01\times 10^{20}$$
  • $$3.01\times 10^{12}$$
  • $$3.01\times 10^{23}$$
  • $$3.01\times 10^{24}$$
In a 2.5 $$L$$ flask at $$27^{\circ}C$$ temperature, the pressure of a gas was found to be 8 $$atm$$. If $$2.41 \times 10^{23}$$ molecules of the same gas are introduced into the container, the temperature changed to $$T_2$$. The pressure of gas is found to be 10 $$atm$$. Find out the value of $$T_2$$:
  • 253 $$K$$
  • 347 $$K$$
  • 230 $$K$$
  • 370 $$K$$
A vessel has x g of gas at high pressure P. When certain gas escapes, the pressure P became P/8 and temperature T became 2T. What is the amount of gas escaped?
  • 2/3 x
  • 1/3 x
  • 15/16 x
  • 3/4 x
The volume of a gas is ______ when the pressure is reduced to half and the absolute temperature is doubled.
  • halved
  • doubled
  • tripled
  • quadrupled
One litre of a gas weighs 2 g at 300 K and 1 atm. If the pressure is made 0.75 atm, at what temperature will one litre of the same gas weigh one gram?
  • 450 K
  • 800 K
  • 600 K
  • 900 K
Which of the following changes cannot increase the volume of a gas by 4 times?
  • T is doubled, P is decreased to half
  • P is kept constant, T is increased by 4 times.
  • P is doubled, T is decreased to half
  • T is kept constant, P is decreased to 1/4th
Choose the correct statement from the following:
  • Molecular collisions are unaffected by gravity.
  • Real gases obey gas laws under any conditions.
  • Gas laws have no significance at absolute zero.
  • At $$0^oC$$, the molecular motion ceases.
The volume occupied by 0.01 moles of helium gas at STP is:
  • $$0.224  l$$
  • $$22.4  l$$
  • $$2240  l$$
  • $$2.24  l$$
The volume occupied by 11 grams of $$CO_2$$ gas at STP is:
  • $$5.6\  l$$
  • $$11.2\  l$$
  • $$22.4\  l$$
  • $$44.8 \ l$$
At sea level air is dense. This is practical application evidence of_________.
  • Boyle's law
  • Charles' law
  • Dalton's law
  • Avogadro's law
The pressure of a gas is due to:
  • Rapid intermolecular collisions
  • Molecular impacts against the walls of vessel
  • Voids between the gas molecules
  • Ideal behaviour of gases
In the reaction $${ N }_{ 2 }+{ 3H }_{ 2 }\longrightarrow { 2H }_{ 3 }$$, ratio by volume of $${ N }_{ 2 },{ H }_{ 2 }$$ and $$ { NH }_{ 3 }$$ is $$1:3:2$$. This illustrates law of :
  • definite proportions
  • multiple proportions
  • reciprocal proportions
  • gaseous proportions
Which are the value of $$R$$ ?
  • $$1.99 \:cal \:deg^{-1} \:mol^{-1}$$
  • $$0.0821 \:litre \:-atm \:deg^{-1} \:mol^{-1}$$
  • $$9.8 \:kcal \:deg^{-1} \:mol^{-1}$$
  • $$8.3 \:joule \:deg^{-1} \:mol^{-1}$$
In the kinetic theory of gases, it is assumed that molecular collisions are :
  • inelastic
  • short in duration
  • one-dimensional
  • not able to exert mutual forces


What conclusion would you draw from the following graphs for an ideal gas?


140971_485877aca811472ab0704ff05c927504.png
  • As the temperature is reduced, the volume as well as pressure increase
  • As the temperature is reduced, the volume becomes zero and the pressure reaches infinity
  • As the temperature is reduced, the pressure decrease
  • A point is reached where, theoretically, the volume become zero
In the equation $$PV=RT$$, the value of $$R$$ will not depend on:
  • the nature of the gas
  • the temperature of the gas
  • the pressure of the gas
  • units of measurement
When an ideal gas undergoes unrestrained expansion, no cooling occurs because of the molecules:
  • are above the inversion temperature.
  • exert no attractive forces on each other.
  • do work equal to loss in kinetic energy.
  • collide without loss of energy.
Scientist, who has important connection with work on gases, was:
  • Boyle
  • Gay Lussac
  • Dalton
  • Faraday
State True or False.
A mixture of ideal gases is cooled upto liquid helium temperature (4.22 K) to form an ideal solution
  • True
  • False
State True or False.
Most of the volume of a container having a gas is empty space.
  • True
  • False
Select the correct answer from the choices given below. 

The three states of matter are classified on the basis of differences of certain _________.
  • chemical properties
  • physical properties
  • physical and chemical properties
  • none of the above
State True or False.
The diameter of molecules are much smaller than the average distance travelled between collisions.
  • True
  • False
$$224\,\, cm^3$$ of ammonia undergoes catalytic oxidation in presence of $$Pt$$ to give nitric oxide and water vapour. The volume of oxygen required for the reaction is:
(All volumes measured at room temperature and pressure)
  • $$896\ cc. of\  O_2$$
  • $$224\ cc. of\  O_2$$
  • $$180\ cc. of \ O_2$$
  • $$280\ cc. of \ O_2$$
The value of molar gas constant is :
  • smaller for compound gases in comparison to other gases
  • different for different gases
  • equal for all gases
  • smaller for elementary gases in comparison to other gases
State True or False.
The mean free path of molecules in gas increases and the number of collisions per unit volume decreases with the lowering of pressure.
  • True
  • False
In the ideal gas equation, the value of universal gas constant depends on :
  • Nature of the gas
  • Pressure of the gas
  • Temperature of the gas
  • Unit of measurement
If saturated vapours are compressed slowly (temperature remains constant) to half the initial volume, their pressure will:
  • become four times
  • become double
  • remain unchanged
  • become half
Select one correct statement. In the gas equation, $$PV= nRT$$
  • $$n$$ is the number of molecules of a gas.
  • $$n$$ moles of the gas have a volume $$V$$.
  • $$V$$ denotes volume of one mole of the gas.
  • $$P$$ is the pressure if the gas when only one mole of gas is present.
Which of the following is not a correct postulate of kinetic theory of gases?
  • The molecules of a gas are continuously moving in different directions with different velocities.
  • The average kinetic energy of the gas molecules is directly proportional to the absolute temperature of the gas.
  • The volume of the gas is due to the large number of molecules present in it.
  • The pressure of the gas is due to the collision of the molecules on the walls of the container.
An ideal gas obeying kinetic theory of gases can be liquefied, if :
  • Its temperature is more than critical temperature $$T_c$$
  • Its pressure is more than critical pressure $$P_c$$
  • Its pressure is more than $$P_c$$ at a temperature less than $$T_c$$
  • It cannot be liquefied at any value of $$P$$ and $$T$$
A drop each of two non-corrosive and non-irritating liquids A and B at a temperature of $$22^{o}C$$ are placed on the skin. Liquid A gives a more cooling sensation than liquid B. Which of the following can be said about the liquids A and B?
  • Liquid A has higher boiling point than that of liquid B.
  • Liquid A has higher latent heat of vaporisation than that of liquid B.
  • Liquid A has lower latent heat of vaporisation than that of liquid B.
  • The boiling points of liquid A and B are equal.
The volume occupied by $$3.5$$ g of $$O_2$$ gas at $$27^o C$$ & $$760 $$ mm pressure is:

[Molecular weight of oxygen $$=16$$ g/mole]
  • $$2.45$$ litres
  • $$5.24$$ litres
  • $$6.4$$ litres
  • $$3.5$$ litres
According to the kinetic theory of gases:
  • Pressure of a gas is due to collisions of molecules with each other
  • Kinetic energy is proportional to square root of the temperature
  • Pressure of a gas is due to collisions of molecules against the sides of the container
  • There is no force of attraction between gas molecules
Statement: Equal volumes of all gases always contain equal number of moles.

State whether the given statement is true or false.
  • True
  • False
State True or False.
Equal volumes of different gases under similar conditions of temperature and pressure contain equal number of atoms.
  • True
  • False
Aqueous tension is the vapour pressure of water and depends only upon temperature.

If the statement is true enter 1, else enter 0.
  • 1
  • 0
  • Both A and B
  • None of these
State True or False.
All the molecules in a given sample of gas move with same speed.
  • True
  • False
An aqueous solution of methanol in water has vapour pressure:
  • equal to that of water
  • equal to that of methanol
  • more than that of water
  • less than that of water
Under the same conditions, two gases have the same number of molecules. They must:
  • be noble gases
  • have equal volumes
  • have a volume of 22.4 dm$$^3$$ each
  • have an equal number of atoms
The total pressure exerted by a mixture of gases is equal to the sum of the partial pressures exerted by each individual gas in the mixture, known as___________
  • Dalton’s law of partial pressure
  • Raoult's law
  • Charle's law
  • Boyle's law
Vapour pressure of a solvent containing nonvolatile solute is_________.
  • more than the vapour pressure of a solvent
  • less than the vapour pressure of solvent
  • equal to the vapour pressure of solvent
  • none
The vapour pressure of a dilute solution of a solute is not influenced by:
  • temperature of solution
  • melting point of solute
  • mole fraction of solute
  • degree of dissociation of solute
Aluminium and coal are examples of solids.
  • True
  • False
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