CBSE Questions for Class 11 Medical Chemistry States Of Matter Gases And Liquids Quiz 4 - MCQExams.com

$$P_{total} = P_{1} + P_{2} + P_{3} + ....$$ 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
Which of the following will diffuse faster than the others?
  • Water
  • Petrol
  • Perfume
  • Milk
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 $$H_2$$
Statement I
The volume of a gas at 100 deg C and 600 mmHg will be lower at STP
Because
Statement II
Decreasing temperature and increasing pressure will cause the volume of a gas to decrease
  • 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.
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
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 shows increasing the kinetic energy of a liquid?
495064.png
  • $$AB$$
  • $$BC$$
  • $$CD$$
  • $$DE$$
  • $$EF$$
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 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
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
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.
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)
  • $$27\ mm\ $$$$\displaystyle Hg$$
  • $$760\ mm\ $$$$\displaystyle Hg$$

  • $$(760-27)\ mm\ Hg $$

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.
An experiment is conducted where droplets of liquid are placed on the surface of a penny. Which of the following substances would you expect to the able to place the maximum number of drops of on the surface of the penny?
  • $$HF$$
  • $$H_{2}O$$
  • $$CH_{3}CH_{2}CHO$$
  • $$CCl_{4}$$
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
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
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
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
The ideal gas law was first stated by:
  • Robert Boyle
  • Jacques Charles
  • Amedeo Avagadro
  • Emile Clapeyron
Which of the following law is followed by ideal gases?
  • Charle's law
  • Boyle's law
  • Avogadro's law
  • All of the above
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
Which of the following are correct for an ideal gas?
  • $${ \left( \cfrac { \partial U }{ \partial V } \right) }_{ T }=0\quad $$
  • $${ \left( \cfrac { \partial H }{ \partial P } \right) }_{ T }=0$$
  • $${ \left( \cfrac { \partial T }{ \partial P } \right) }_{ H }=0\quad $$
  • $${ \left( \cfrac { \partial P }{ \partial T } \right) }_{ H }=0\quad $$
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
At $$25^oC$$, the vapour pressure of pure benzene is 100 torr, while that of pure ethyl alcohol is 44 torr. Assuming ideal behaviour, calculate the vapour pressure at $$25^oC$$ of a solution which contains 10 g of each substance.
  • 33.775 torr
  • 54.775 torr
  • 64.775 torr
  • 60.775 torr
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
Mole fraction of the component A in vapour phase is $$x_1$$ and mole fraction of component A in liquid mixture is $$x_2$$, then ($$p^0_A =$$ vapour pressure of pure A; $$p^0_B =$$ vapour pressure of pure B), the total vapour pressure of liquid mixture is :
  • $$p^0_A\dfrac{x_2}{x_1}$$
  • $$p^0_A\dfrac{x_1}{x_2}$$
  • $$p^0_B\dfrac{x_1}{x_2}$$
  • $$p^0_B\dfrac{x_2}{x_1}$$
If the concentration of water vapour in the air is $$1\%$$ and the total atmospheric pressure equals $$1$$atm then the partial pressure of water vapour is?
  • $$0.1$$ atm
  • $$1$$ mm Hg
  • $$7.6$$ mm Hg
  • $$100$$ atm
The following graphs illustrate: 
667491_7f8051aff01e4c1ea89d2564e5a42584.png
  • Dalton's law
  • Boyle's law
  • Charles' law
  • Gay-Lussac's law
The temperature, at which the density of $$O_{2}$$ at $$1\ atm$$, is the same as that of $$CH_{4}$$ at S.T.P is:
  • $$273^{\circ}C$$
  • $$100^{\circ}C$$
  • $$546^{\circ}C$$
  • $$150^{\circ}C$$
What is the vapour pressure of a solution of glucose which has an osmotic pressure of 3 atmospheres at $$20^C?$$ The vapour pressure of water at $$20^oC$$ is $$17.39 mm$$. Consider the density of solution equal to that of the solvent.
  • $$12.35 mm$$
  • $$14.35 mm$$
  • $$16.35 mm$$
  • $$17.35 mm$$
At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure?

[Mol weight: $$NaCl=58.5,{ H }_{ 2 }{ SO }_{ 4 }=98.0g.{ mol }^{ -1 }$$]
  • $$1$$ molal $$NaCl$$
  • $$1$$ molar $$NaCl$$
  • $$1$$ molal $${H}_{2}{SO}_{4}$$
  • $$1$$ molar $${H}_{2}{SO}_{4}$$
Which of the following do not pertain to the postulates of kinetic theory of gases?
  • The gas molecules are perfectly elastic
  • Speed of gas molecules are every changing
  • Pressure exerted by the gas is due to the collision of molecules with the walls of the container
  • Kinetic energy of a gas is given by the sum of $$273$$ and temperature in Celsius scale
Plot of Maxwell's distribution of velocities is given below:
which of following is correct?
654454_eb65a8304fc646848f5db3cffddaa3ec.png
  • $$T_{1} > T_{2}$$
  • $$T_{1} < T_{2}$$
  • $$v_{1} < v_{2}$$
  • $$f_{1} > f_{2}$$
Which of the following property indicates weak intermolecular forces of attraction in liquid?
  • High heat of vaporization
  • High vapour pressure
  • High critical temperature
  • High boiling point
At $$27^{\circ}C$$ a sample of ammonia gas exerts a pressure of $$5.3\ atm$$. What is the pressure when the volume of the gas is reduced to one-tenth of the original value at the same temperature?
  • $$0.53\ atm$$
  • $$5.3\ atm$$
  • $$53\ atm$$
  • None of these
Equal weights of two gases of molecular weight $$4$$ and $$40$$ are mixed. The pressure of the mixture is $$1.1$$ atm. The partial pressure of the light gas in this mixture is :
  • $$0.55$$ atm
  • $$0.15$$ atm
  • $$1$$ atm
  • $$0.11$$ atm
On the surface of the earth at $$1\ atm$$ pressure, a balloon filled with $$H_{2}$$ gas occupies $$500\ mL$$. This volume is $$5/6$$ of its maximum capacity. The balloon is left in air. It starts rising. The height above which the balloon will burst if temperature of the atmosphere remains constant and the pressure decreases $$1\ mm$$ for every $$100\ cm$$ rise of height is:
  • $$120\ m$$
  • $$136.67\ m$$
  • $$126\ m$$
  • $$100\ m$$
'a' moles of $$PCl_5$$, undergoes, the thermal dissociation as: $$PCl_5\rightleftharpoons PCl_3+Cl_2$$, the mole fraction of $$PCl_3$$ at equilibrium is $$0.25$$ and the total pressure is $$2.0$$ atmosphere. The partial pressure of $$Cl_2$$ at equilibrium is?
  • $$2.5$$
  • $$1.0$$
  • $$0.5$$
  • None
The two bulbs of volume $$5$$ litre and $$10$$ litre containing an ideal gas at $$9\ atm$$ and $$6\ atm$$ respectively are connected. What is the final pressure in the two bulbs if the temperature remains constant ? 
  • $$15\ atm$$
  • $$7\ atm$$
  • $$12\ atm$$
  • $$21\ atm$$
Assume that you take a flask, evacuate it to remove all the air and find it's mass to be 478.1 g .You then fill the flask with argon to a pressure of 2.15 atm and reweigh it. What would the balance read (in grams) of the flask has a volume of 7.35 L and the temperature is $$ 20^0 C$$ ?
  • 203.6 g
  • 504.3 g
  • 471.1 g
  • None of these
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