CBSE Questions for Class 11 Engineering Chemistry States Of Matter Quiz 10 - MCQExams.com

Select the incorrect order of boiling point between the following compounds :
  • $$N_3H < CH_3N_3$$
  • $$Me_2SO_4 < H_2SO_4$$
  • $$Me_3BO_3 < B(OH)_3$$
  • $$BF_3 < BI_3$$
Which of the following statements are false? Rewrite them correctly.

Volume remaining constant, the pressure is inversely proportional to temperature in degrees kelvin.
  • True
  • False
At a certain pressure, volume of the gas at $$27^\circ C$$ is $$20$$ litre. If the pressure and temperature are doubled, the volume will be 
  • $$40\,litre$$
  • $$20\,litre$$
  • $$10.9\,litre$$
  • $$8.2\,litre$$
Which of the following curve does not represent Gay lusacc's law?
"Equal volumes of all gases at the same temperature and pressure contain equal number of particles." This statement is a direct consequence of:
  • Avogadro's law
  • Charles law
  • Ideal gas equation
  • Law of partial pressure
The equation of state for $$5$$ g of oxygen at a pressure $$P$$ and temperature $$T$$, when occupying a volume $$V$$, will be:
  • $$PV = 5 RT$$
  • $$PV = \left (\dfrac{5} {2} \right ) RT$$
  • $$PV = \left (\dfrac{5} {16} \right ) RT$$
  • $$PV = \left (\dfrac{5} {32} \right ) RT$$
According to the kinetic theory of gases, in an ideal gas, between two successive collisions, a gas molecule travels:
  • in a wavy path
  • in a straight line path
  • with an accelerated velocity
  • in a circular path
Match the following :
List -IList-II
A. Boyle’s law$$P_{wet}=P_{dry}+P_{water\ vapour}$$
B. Avogadro law$$V_{1}=n_{1}\left ( \dfrac{V_{2}}{n_{2}} \right )$$
C. Charles law$$V_{1}=V_{0}\left (1+ \dfrac{t}{273} \right )$$
D. Dalton’s law$$V_{1}=P_{2}\left ( \dfrac{V_{2}}{P_{1}} \right )$$
The correct match is:
  • A-1, B-2, C-3, D-4
  • A-2, B-3, C-4, D-1
  • A-4, B-3, C-2, D-1
  • A-4, B-2, C-3, D-1
2.5 L of a sample of a gas at $$27^\circ C$$ and 1 bar pressure is compressed to a volume of 500 mL keeping the temperature constant, the percentage increase in the pressure is :
  • 100%
  • 400%
  • 500%
  • 80%
Dalton's law of partial pressures is not applicable to which one of the following?
  • $$H_{2}+Cl_{2}$$
  • $$SO_{2}+Cl_{2}$$
  • $$NH_{3}+HCl$$
  • All the above
Which of the following statement(s) is/are correct ?
  • At $$273^{o}C$$, the volume of a given mass of a gas will be twice its volume at $$0^{o}C$$ and $$1$$ atm pressure
  • At $$-136.5^{o}C$$, the volume of a given mass of a gas will be half its volume at $$0^{o}C$$ and 1 atm pressure
  • The mass ratio of equal volumes of $$NH_{3}$$ and $$H_{2}S$$ under identical conditions of temperature and pressure is $$1:2$$
  • The molar ratio of equal masses of $$CH_{4}$$ and $$SO_{2}$$ is $$4:1$$
A gas is collected by downward displacement of water. Select the correct expression for $$P_{gas}$$ according to the diagram. [Density of Hg (l) $$= 13.6 \ g/cm^3]$$

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  • $$P_{gas}=P_{atmp}-\left [ aq.tension+\dfrac{h}{13.6} \right ]$$
  • $$P_{gas}=P_{atm}-h \rho g$$
  • $$P_{gas}=P_{atmp}-aq.tension+\dfrac{h}{13.6}$$
  • None of these
Which of the following is the only incorrect informarion regarding the composition of the system at 0.51 bar pressure ?
  • $$ X_A = 0.45 $$
  • $$ Y_A = \frac {6}{17} $$
  • $$ n_{A(liquid) } = \frac {12}{11} $$
  • $$ n_{A(vapour) } = \frac {12}{11} $$
At the same temperature, HCl gas and NH$$_{3}$$ gas are present in two vessels of same volume at a pressure of 'P' atmospheres each. When one jar is inverted over the other so that the two will mix, after some time the pressure in the vessels will become:
  • $$\cfrac{P}{2}$$
  • $$\cfrac{P}{4}$$
  • Zero
  • P
An open vessel at $$27^oC$$ is heated until the three-fourths mass of the air in it has been expelled. Neglecting the expansion of the vessel, find the temperature to which the vessel has been heated.
  • $$T_2=723^oC$$
  • $$T_2=958^oC$$
  • $$T_2=927^oC$$
  • None of these
$$45.4$$ L of dinitrogen reacted with $$22.7$$ L of dioxygen and $$45.4$$ L of nitrous oxide was formed. The reaction is given below:
$$\displaystyle 2N_{2}\left ( g \right )+O_{2}\left ( g \right )\rightarrow 2N_{2}O\left ( g \right )$$
Which law is being obeyed in this experiment?
  • Gay Lussac's law of gaseous volumes
  • Henry's Law
  • Raoult's Law
  • None
Gay-Lussac's law i.e, dependence of pressure of ideal gas with temperature in $$^oC$$ can be expressed as $$P_t=a+bt$$ where
  • $$a=P_0$$ and t in $$^oC$$
  • $$b=\left (\frac {\partial P}{\partial t}\right )_V$$
  • $$b=\left [\frac {P_0}{273.15}\right ]$$
  • $$P_T=KT$$, where T is in K
Two identical vessels are filled with 44 g of hydrogen and 44 g of carbon dioxide at the same temperature. If pressure of $$CO_2$$ is 2 atm. Find the pressure of hydrogen.
  • $$P_{H_2}=56\ atm$$
  • $$P_{H_2}=44\ atm$$
  • $$P_{H_2}=32\ atm$$
  • None of these
A zinc metal sample containing zinc chloride as impurity was made to react with an excess of dilute hydrochloric acid at $$ 27^{o}C$$. Liberated hydrogen gas is collected at 760 mm Hg pressure that occupies $$780.0 cm^{3}$$ volume. If the vapour pressure of water at $$27^{o}C$$ is 14 mm Hg, what is the volume of $$H_{2}$$ at STP? The Standard pressure is 760 mm Hg (molar volume of gas at standard temperature and pressure, $$STP = 22.4 dm^{3}$$)
  • $$746 cm^{3}$$
  • $$697 cm^{3}$$
  • $$750 cm^{3}$$
  • $$300 cm^{3}$$
At constant temperature, the pressure of a gas is __________ to its volume.
  • inversely proportional
  • directly proportional
  • not proportional
  • none of the above
In the reaction $$N_{2}+3H_{2}\rightarrow 2NH_{3} $$, the ratio by volume of $$N_{2},\ H_{2} \:$$ and$$\: NH_{3}$$ is $$1 : 3 : 2$$. 

This illustrates the law of:
  • definite proportion
  • multiple proportion
  • reciprocal proportion
  • gaseous volumes
To which of the following mixtures Dalton's law is not applicable?
  • $$CO_2$$ and CO at room temperature
  • Ammonia and hydrogen chloride at room temperature
  • $$NH_3$$ and steam at room temperature
  • He and $$H_2$$
A balloon containing 1 mole air at 1 $$atm$$ initially is filled further with air till pressure increases to 4 $$atm$$. The initial diameter of the balloon is 1 $$m$$ and the pressure at each stage is proportion to diameter of the balloon. How many no.of moles of air added to change the pressure from 1 $$atm$$ to 4 $$atm$$.
  • 80
  • 257
  • 255
  • 256
The number of effusion steps required to convert a mixture of $$H_2$$ and $$O_2$$ from 240 : 1600 (by mass) to 3072 : 20 (by mass) is:
  • 2
  • 4
  • 5
  • 6
Vapour pressure of $$CC{l}_{4}$$ at $$25^{O}C$$ is 143mm Hg. 0.5gm of a non-volatile solute (mol. wt. 65) is dissolved in 100ml of $$CC{l}_{4}$$. Find the vapour pressure of the solution.
(Density of $$CC{l}_{4} = 1.58 gm/{cm}^{3}$$)
  • 141.93 mm
  • 94.39 mm
  • 199.34 mm
  • 143.99 mm
Ideal gas has a volume of 10 litres at $$20^oC$$ and a pressure of 750 $$mm$$ $$Hg$$. Find the expressions which is needed  to determine the volume of the same amount of gas at $$STP$$?
  • $$\displaystyle 10 \times \frac{750}{760} \times \frac{0}{20}L$$
  • $$\displaystyle 10 \times \frac{750}{760} \times \frac{293}{273}L$$
  • $$\displaystyle 10 \times \frac{760}{750} \times \frac{0}{20}L$$
  • $$\displaystyle 10 \times \frac{760}{750} \times \frac{273}{293}L$$
  • $$\displaystyle 10 \times \frac{750}{760} \times \frac{273}{293}L$$
"All gases have the same number of moles in the same volume at constant temperature and pressure:. This statments belongs to :
  • Boyle's law
  • Charles's law
  • Avogadro's principle
  • ideal gas law
  • Dalton's law
Statement 1 : In the kinetic theory of gases, collisions between gas particles and the walls of the container are considered elastic.
Statement 2 : Gas molecules are considered point like, volume less particles with no inter molecular forces and in constant, random motion.

  • Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.

  • Both 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.

''Total pressure of a gaseous mix is equal to the sum of the partial pressures'', this statement is from : 
  • Boyle's law
  • Charles's law
  • Avogadro's principle
  • ideal gas law
  • Dalton's law
Inelastic collisions occur in :
I. Real gases
II. Ideal gases
III. Fusion reactions
Which of the following is correct option about the above problem?
  • I and II
  • II and III
  • I and III
  • I only
  • II only
Statement 1: At the same temperature and pressure, 1 L of hydrogen gas and  1 L of neon gas have the same mass.
Statement 2: Equal volumes of ideal gases at the same temperature and pressure contain the same number of moles.

  • Both statement 1 and statement 2 are correct and statement 2 is the correct explanation of statement 1

  • Both statement 1 and statement 2 are correct but Statement 2 is not the correct explanation of Statement 1

  • Statement 1 is correct but statement 2 is incorrect

  • Statement 1 is incorrect but statement 2 is correct

  • Both the statement 1 and statement 2 are incorrect

Among the following which one shows  that the total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases.
  • V/T$$=$$k
  • P/T$$=$$k
  • PV$$=$$k
  • $$P_T=P_1+P_2+P_3$$
  • PT$$=$$k
Equal weights of $$CH_{4}$$ and $$H_{2}$$ are mixed in an empty container at $$25^{\circ}C$$. The fraction of the total pressure exerted by $$H_{2}$$ is:
  • $$1/9$$
  • $$1/2$$
  • $$8/9$$
  • $$16/17$$
All of the following statements are related to the kinetic molecule theory of gases except:
  • gas molecules have no inter-molecular forces
  • gas particles are in random motion
  • the collisions between gas particles are elastic
  • gas particles have no volume
  • the average kinetic energy is proportional to the celsius temperature of the gas
Statement I : At STP, 22.4 liters of He will have the same volume as one mole of $$\displaystyle { H }_{ 2 }$$ (assume ideal gases).
Statement II : One mole or 22.4 liters of any gas at STP will have the same mass.
  • true, false
  • false, true
  • true, true, correct explanation
  • true, true, not correct explanation
$$CuSO_4$$$$\cdot$$$$5H_2O(s)$$$$\rightleftharpoons$$ $$CuSO_4\cdot$$ 3$$H_2O(s)$$ + $$2H_2O(g)$$; $$K_p$$ = 4$$\times10^{-4}$$ $$atm^2$$ if the vapour pressure of water is 38 torr then percentage of relative humidity is: ( Assume all data at constant temperature)
  • $$4$$
  • $$10$$
  • $$40$$
  • $$none\ of\ these$$
What is the effect on the pressure of a gas if its temperature is increased at constant volume?
  • The pressure of the gas increases
  • The pressure of the gas decreases
  • The pressure of the gas remains same
  • The pressure of the gas becomes double
Two liquids $$X$$ and $$Y$$ form an ideal solution at $$300\ K$$, the vapour pressure of the solution containing $$1\ mole$$ of $$X$$ and $$3\ moles$$ of $$Y$$ is $$550$$ mm Hg. At the same temperature, if $$1\ mole$$ of $$Y$$ is further added to this solution, the vapour pressure of the solution increases by $$10\ mm\ Hg$$. Vapour pressure (in mm Hg) of $$X$$ and $$Y$$ in their pure states will be respectively :
  • $$200$$ and $$300$$
  • $$300$$ and $$400$$
  • $$400$$ and $$600$$
  • $$500$$ and $$600$$
The vapour pressures of two liquids A and B in their pure states are in the ratio of 1 :A binary solution of A and B contains A and B in the mole proportion of 1 :The mole fraction of A in the vapour phase of the solution will be:
  • $$0.33$$
  • $$0.2$$
  • $$0.25$$
  • $$0.52$$
Calculate the temperature at which the root mean square velocity of chlorine gas molecules is twice the root mean square velocity of carbon dioxide gas molecules at $$40^0C$$.
  • $$500 K$$
  • $$1000 K$$
  • $$1500 K$$
  • $$2000 K$$
Ideal gases:
  • have forces of attraction between them
  • are always linear in shape
  • never travel with a straight line motion
  • have molecules that are close together
  • have low masses and are spread far apart
Which of the following shows behavior of binary liquid solution?
  • Plot of $${ 1 }/{ { \rho }_{ total } }$$ vs $${ 1 }/{ { Y }_{ A } }$$, mole fraction of $$A$$ in vapour phase
  • Plot of $${ 1 }/{ { \rho }_{ total } }$$ vs $${ 1 }/{ { Y }_{ B } }$$ is linear 
  • Plot of $${ 1 }/{ { \rho }_{ total } }$$ vs $${ 1 }/{( { Y }_{ B } {Y}_{A})}$$ is linear
  • Plot of $${ 1 }/{ { \rho }_{ total } }$$ vs $${ Y }_{ A }$$ is linear
When a liquid that is immiscible with water was steam distilled at $$95.2^o$$C at a total pressure of $$99.652$$ kPa, the distillate contained $$1.27$$ g of the liquid per gram of water. What will be the molar mass of the liquid if the vapour pressure of water is $$85.140$$ kPa at $$95.2^o$$C?
  • $$99.65\ g mol^{-1}$$
  • $$18 \ g mol^{-1}$$
  • $$134.1 \ g mol^{-1}$$
  • $$105.74\ g mol^{-1}$$
To use Gay-Lussac's Law, which of the following needs to remain constant?
  • Volume and the number of moles of a gas
  • Pressure and temperature
  • Temperature and the number of moles of a gas
  • Pressure and the number of moles of a gas
  • Temperature and volume
Avogadro's law shows the relationship between which two variables?
  • Volume and number of moles
  • Pressure and number of moles
  • Volume and pressure
  • Temperature and pressure
  • Temperature and number of moles
When $$100\ ml$$ of a $$O_{2} - O_{3}$$ mixture was passed through turpentine, there was reduction of volume by $$20\ mL$$. If $$100\ ml$$ of such a mixture is heated, what will be the increase in volume?
  • 10%
  • 20%
  • 40%
  • 30%
An ideal gas: 
  • Has no intermolecular attraction
  • Molecules do not collide with each other
  • The product of P and V is constant at a fixed temperature for definite mass
  • Can be liquefied easily
If the vapour are compressed slowly and isothermally , at what pressure , the first drop of liquid will appear ?
  • 0.4 bar
  • 0. 5 bar
  • 0.52 bar
  • 0.6 bar
Two liquids $$X$$ and $$Y$$ from an ideal solution. At $$300K$$, a vapour pressure of the solution containing $$1$$ mol of $$X$$ and $$3$$ mol of $$Y$$ is $$550$$ $$mm \ Hg$$. At the same temperature, if $$1$$ mol of $$Y$$ is further added to this solution, a vapour pressure of the solution increased by $$10$$ $$mm \ Hg$$. Vapour pressure ( in mmHg) of $$X$$ and $$Y$$ in their pure states will be respectively: 
  • $$300$$ and $$400$$
  • $$400$$ and $$600$$
  • $$500$$ and $$600$$
  • $$200$$ and $$300$$
At certain temperature ($$T$$) for the gas phase reaction
$$2{ H }_{ 2 }O(g)+2{ Cl }_{ 2 }(g)\rightleftharpoons 4HCl(g)+{ O }_{ 2 }(g);{ K }_{ P }=12\times { 10 }^{ 8 }atm$$
If $${Cl}_{2}$$, $$HCl$$ and $${O}_{2}$$ are mixed in such a manner that the partial pressure of each is $$2atm$$ and the mixture is brough into contact with excess of liquid water. What would be approximate partial pressure of $${Cl}_{2}$$ when equilibrium is attained at temperature ($$T$$)?
[Given:Vapour pressure of water is $$380mm$$ $$Hg$$ at temperature ($$T$$)]
  • $$3.6\times { 10 }^{ -5 }atm$$
  • $${ 10 }^{ -4 }atm$$
  • $$3.6\times { 10 }^{ -3 }atm$$
  • $$0.01$$atm
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