CBSE Questions for Class 11 Engineering Chemistry States Of Matter Quiz 3 - MCQExams.com

The $$CO_{2}$$ gas does not follow gaseous laws at all ranges of pressure and temperature because :
  • It is triatomic gas
  • Its internal energy is quite high
  • There is attraction between its molecules
  • It solidity at low temperature
The molar volume of $$CO_2$$ is maximum at: 
  • $$NTP$$
  • $$0^o\ C$$ and $$2.0\ atm$$
  • $$127^o\ C$$ and $$1\ atm$$
  • $$273^o\ C$$ and $$2\ atm$$
By ideal gas law, find the approximate volume that will be occupied by 0.5 mole of an ideal gas at 30$$^oC$$ and 3 $$atm$$ pressure (gas constant $$R$$ $$=$$ 0.0821 $$L atm / \:mol / \: K$$)?
  • Less than 1 $$L$$
  • 5 $$L$$
  • 10 $$L$$
  • 15 $$L$$
  • More than 20 $$L$$
Find the new volume of the gas, when kelvin temperature and pressure of a fixed amount of gas is doubled?
  • Twice its original volume
  • Unchanged
  • One-half its original volume
  • One-fourth its original volum
  • Four times greater than its original volume
According to the Kinetic-Molecular Theory, the kinetic energy of the molecules increases when they are --------------
  • mixed with other molecules at lower temperature
  •  frozen into a solid
  •  condensed into a liquid
  •  heated to a higher temperature
  • Collide with each other in a container at a lower temperature
Which one proposes a relationship between the combining volumes of gases with respect to the reactants and gaseous products.
  • Avogadro's number
  • $$P_1V_1=P_2V_2$$
  • $$V_1T_2=V_2T_1$$
  • Dalton's Theory
  • Gay-Lussac's Law
PV $$=$$ nRT is the equation for:
  • Boyle's law
  • Charle's law
  • Ideal gas equation
  • Combined gas law
  • Dalton's law of partial pressures
$$P_{total} = P_{1} + P_{2} + P_{3} + ....$$ which of the following is correct about the expression?
  • Boyle's law
  • Charle's law
  • Ideal gas equation
  • Combined gas law
  • Dalton's law of partial pressures
Five litres of gas at $$STP$$ have a mass of 12.5 $$g$$.What is the molecular mass of the gas?
  • 12.5 $$g/mol$$
  • 25.0 $$g/mol$$
  • 47.5 $$g/mol$$
  • 56.0 $$g/mol$$
  • 125 $$g/mol$$
A gas is confined in the manometer as shown below. The stopcock is then opened and the highest level of mercury inside the tube moved to a level that is 80 $$mm$$ above its lowest level. What is the pressure of the gas? 
487483_b42e383f2d9443fa9991788594fb021c.png
  • 80 $$mm \:Hg$$
  • 160 $$mm \:Hg$$
  • 680 $$mm \:Hg$$
  • 840 $$mm \:Hg$$
  • Cannot be determined
Which of the following pair of gases cannot be separated by diffusion method?
  • $$SO_2$$ and $$H_2$$
  • $$CO_2$$ and $$N_2O$$
  • $$NH_3$$ and $$N_2$$
  • $$CO_2$$ and $$H_2$$
All gases have the same number of moles in the same volume at constant T and P is stated by :
  • Boyle's law
  • Charle's law
  • Avogardro's law
  • ideal gas law
  • Dalton's law
Regarding the kinetic molecular theory, which of the following statement is not true?
  • The volume that gas molecules occupy is negligible compared to the volume within which the gas is contained
  • There are no forces present between gas molecules
  • Collisions between gas molecules are perfectly elastic
  • Gas molecules travel in a continuous, random motion
  • The average kinetic energy of gas molecules is inversely proportional to temperature
The total pressure of a gaseous mixture is equalto the sum of the partial pressures is:
  • Boyles law
  • Charles law
  • Avogadro's law
  • Ideal gas law
  • Daltons law
Which one is correct about  Gay-Lussac's law?
  • V/T $$=$$ k
  • P/T $$=$$ k
  • PV $$=$$ k
  • $$P_T=P_1+P_2+P_3$$
  • PT $$=$$ k
Calculate the number of iron atoms in a piece of iron weighing $$2.8 g$$. (Atomic mass of iron $$=56$$)
  • $$30.11\times { 10 }^{ 23 }$$ atoms
  • $$3.11\times { 10 }^{ 23 }$$ atoms
  • $$3.0115\times { 10 }^{ 22 }$$ atoms
  • $$301.1\times { 10 }^{ 23 }$$ atoms
Gay Lussac's Law of combining volumes is applicable for combustion of carbon.
  • True
  • False
64 g of sulphur dioxide occupies $$22.4\ L$$ volume at STP.
  • True
  • False
The value of the Avogadro constant is:
  • $$6.022 \times 10^{13}$$
  • $$6.022 \times 10^{22}$$
  • $$6.022 \times 10^{23}$$
  • $$6.022 \times 10^{24}$$
Which gas law uses pressure, number of moles, temperature, volume and the gas constant (R)?
  • Boyle's Law
  • Ideal Gas Law
  • Combined Gas Law
  • Charles' Law
Which statement is NOT compatible with the ideal gas law?
  • Gas particles have no definite volume
  • Gas temperature depends on particles mass and velocity
  • Gas particles are in constant, random motion
  • Gas particles have no mass
Drops are water are created due to-
  • air resistance
  • surface tension
  • gravity
  • all of these
Statement I: In the kinetic theory of gases, collisions between gas particles and the walls of the container are considered elastic.
Statement II: Gas molecules are considered pointlike, volumeless particles with no intermolecular forces and in constant, random motion.
  • Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1
  • Both the Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1
  • Statement 1 is correct but Statement 2 is not correct
  • Statement 1 is not correct but Statement 2 is correct
  • Both the Statement 1 and Statement 2 are not correct
Which of the following is a possible source of error in the results of this experiment?
524223_36298f57589f4772952ec05e1b2c5e37.png
  • Inaccurate weighing of the isopropanol
  • The presence of bits of broken glass in the flask
  • Failure to correct for humidity
  • Misreading of the atmospheric pressure
Two gases A and B are taken in same volume containers under similar conditions of temperature and pressure. In container A, there are '2N' molecules of gas A. How many number molecules does container B have? 
  • 2N
  • 4N
  • N
  • 8N
If the gas particles in a rigid container slow down, what will happen to the pressure inside the container?
  • Pressure will increase
  • Pressure will decrease
  • Pressure will oscillate
  • Pressure will not change
The initial pressure inside the flask is:
524221_18c042995fb147b9a377600f147d827d.png
  • near zero (vacuum)
  • $$27\ mm\ $$$$\displaystyle Hg$$
  • $$760\ mm\ $$$$\displaystyle Hg$$

  • $$(760-27)\ mm\ Hg $$

Which gas law is summarized with the following equation?
$$({P}_{1}{V}_{1})/{T}_{1}=({P}_{2}{V}_{2})/{T}_{2}$$
  • Boyle's Law
  • Ideal Gas Law
  • Combined Gas Law
  • Charles; Law
Identify which of the following statements is FALSE?
  • The vapor pressure of a liquid decreases with increasing atmospheric pressure.
  • The value of an equilibrium constant is dependent on temperature.
  • The rate of a spontaneous reaction cannot be determined solely by its Gibbs free energy.
  • During a phase transition, the temperature of a substance must be constant.
  • The addition of a catalyst to a reaction at equilibrium has no net effect on the system.
The mass of a non-volatile solute of molar mass 40 g $$mol^{-1}$$ that should be dissolved in 114 g of octane to lower its vapour pressure by 20% is :
  • 10 g
  • 11.4 g
  • 9.8 g
  • 12.8 g
Which of the following has more surface tension at same temperature?
  • Water
  • Mercury
  • Ethanol
  • Glycerin
When applied to law of combining volumes, which of the following is correct about Berzelius hypothesis ?
a) it predicts atoms are indivisible
b)it predicts atoms are divisible
c)it is contrary to Dalton's hypothesis
  • Only a
  • Only b
  • Both a and c
  • Both b and c
At constant temperature, the behavior of a real gas more closely approximates that of an ideal as its volume increases due to which of the following?
  • The average molecular kinetic energy decreases.
  • The molecules have expanded.
  • The average molecular speed decreases.
  • The average distance between the molecules becomes greater.
The ideal gas law was first stated by:
  • Robert Boyle
  • Jacques Charles
  • Amedeo Avagadro
  • Emile Clapeyron
Surface tension is responsible for
  • Lower layer of water has lower veocity
  • A small needle can be made to float on the surface of water
  • Higher layer of water has lower veocity
  • None of these
Just because you mix two things together does not necessarily mean they will form a homogeneous mixture (a solution). For example, if you add sodium chloride, $$NaCl$$, to a container that has both hexane and water, the $$NaCl$$ will dissolve into the water, but will not be found in the hexane $$C_{6}H_{14}$$.
Which of the following statement BEST explains these observations?
  • Polar water molecules form ion-dipole forces with the ions of $$NaCl$$. Hexane, being nonpolar, cannot form these ion-dipole interactions.
  • Nonpolar hexane molecules tend to repel the ions that make up $$NaCl$$.
  • Nonpolar hexane is less dense that water, so when the two are in the same container, any $$NaCl$$ that is added to the mixture sinks to the bottom of the container and cannot get into the hexane layer.
  • Nonpolar hexane molecules and water molecules repel one another.
Small insects such as the water strider can walk on water due to which phenomenon (Choose the best one) 
  • viscosity
  • surface tension
  • friction
  • none of these
If common salt is dissolved in water, then the Surface Tension of salt water is
  • Increased
  • Decreased
  • Not changed
  • First decreases and then increases
For a non-volatile solute:
  • vapour pressure of solution is more than vapour pressure of solvent
  • vapour pressure of solvent is zero
  • vapour pressure of solute is zero
  • all of the above
Surface tension may be defined as
  • The work done per unit area in increasing the surface area of a liquid under isothermal condition
  • The work done per unit area in increasing the surface area of a liquid under adiabatic condition
  • The work done per unit area in increasing the surface is of a liquid under both isothermal and adiabatic conditions.
  • Free surface energy per init volume
At critical temperature, the surface tension of a liquid is
  • zero
  • infinity
  • the same as that at any other temperature
  • Can not be determined
Rain drops are spherical in shape because of
  • Surface tension
  • Capillary
  • Downward motion
  • Acceleration due to gravity
Choose the wrong statement from the following?
  • Small droplets of a liquid are spherical due to surface tension
  • Oil rises through the wick due to capillarity
  • In drinking the cold drinks through a straw, we use the phenomenon of capillarity
  • Gum is used to stick two surfaces. In this process we use the property of Adhesion
The vapour pressure of pure benzene at $$88^oC$$ is 957 mm and that of toluene at the same temperature is 379.5 mm. Calculate the composition of benzene-toluene mixture boiling at $$88^oC$$.
  • $$x_{benzene}=0.66; \,x_{toluene}=0.34$$
  • $$x_{benzene}=0.34; \,x_{toluene}=0.66$$
  • $$x_{benzene} = x_{toluene}=0.5$$
  • $$x_{benzene}=0.75;\, x_{toluene}=0.25$$
The specific heat of a bivalent metal is 0.The approximate equivalent mass of the metal will be:
  • 40
  • 20
  • 80
  • 10
Four flasks of 1 litre capacity each arc separately filled with gases $$H_2, He, O_2$$ and $$O_3$$. At the same temperature and pressure the ratio of the number of atoms of these gases present in different flasks would be: 
  • 1 : 1 : 1 : 1
  • 2 : 1 : 2 : 3
  • 1 : 2 : 1 : 3
  • 3 : 2 : 2 : 1
Vapour pressure of pure $$A(p^0_A)=100$$ mm Hg
Vapour pressure of pure $$B(p^0_B)=150$$ mm Hg

2 mole of liquid A and 3 mole of liquid B are mixed to form an ideal solution. The vapour pressure of the solution will be :
  • 135 mm
  • 130 mm
  • 140 mm
  • 145 mm
In the reaction, $$N_2 + 3H_2 \rightarrow 2NH_3$$, the ratio of volumes of nitrogen, hydrogen and ammonia is 1 : 3:These figures illustrate the law of: 
  • constant proportions
  • Gay-Lussac
  • multiple proportions
  • reciprocal proportions
At $$25^oC$$, the total pressure of an ideal solution obtained by mixing 3 mole of A and 2 mole of B, is 184 torr. What is the vapour pressure (in torr) of pure B at the same temperature (Vapour pressure of pure A at $$25^oC$$ is 200 torr.)?
  • 180
  • 160
  • 16
  • 100
Equal volumes of different gases at any definite temperature and pressure have:
  • equal weights
  • equal masses
  • equal densities
  • equal number of moles
0:0:1


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