CBSE Questions for Class 11 Medical Chemistry States Of Matter Gases And Liquids Quiz 10 - MCQExams.com

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) $$= 13.6 \ g/cm^3]$$

75254.jpg
  • $$P_{gas}=P_{atmp}-\left [ aq.tension+\dfrac{h}{13.6} \right ]$$
  • $$P_{gas}=P_{atm}-h \rho g$$
  • $$P_{gas}=P_{atmp}-aq.tension+\dfrac{h}{13.6}$$
  • None of these
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
Calculate the volume of $$CO_{2}$$ evolved by the combustion of $$50$$ ml of a mixture containing $$40$$ per $$C_{2}H_{4}$$ and $$60$$ per $$CH_{4}$$ (by volume).
  • $$70$$ ml
  • $$75$$ ml
  • $$80$$ ml
  • $$82$$ ml
The pressure exerted by saturated water vapour is called aqueous tension. The pressure of the dry gas can be calculated as?
  • $$\displaystyle P_{Dry \: gas}=P_{Total}-$$ aqueous tension
  • $$\displaystyle P_{Dry \: gas}=P_{Total}+$$ aqueous tension
  • $$\displaystyle P_{Dry \: gas}=P_{Total}/$$ aqueous tension
  • $$\displaystyle P_{Dry \: gas}=P_{Total}*$$ aqueous tension
$$45.4$$ 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?
  • Henry's Law
  • Gay Lussac's law of gaseous volumes
  • Raoult's Law
  • None
Calculate the mean free path in $$\displaystyle CO_{2}$$ at $$\displaystyle 27^{\circ}C$$ and a pressure of $$\displaystyle 10^{-9}$$ bar. Molecular diameter of $$CO_2$$ is $$500$$ pm.
[ Given : R $$\displaystyle =\frac{25}{3}$$ $$\displaystyle J.mol^{-1}K^{-1}, \sqrt{2}=1.4, \pi =\frac{22}{7}, N_{A}=6\times 10^{23}$$]
  • $$\displaystyle 3.788\times 10^{3}$$ cm
  • $$\displaystyle 7.47\times 10^{3}$$ cm
  • $$\displaystyle 6.43\times 10^{5}$$ cm
  • None of these
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, $$STP = 22.4 dm^{3}$$)
  • $$746 cm^{3}$$
  • $$697 cm^{3}$$
  • $$750 cm^{3}$$
  • $$300 cm^{3}$$
According to kinetic theory of gases:
  • Collisions are always elastic.
  • Heavier molecules transfer more momentum to the walls of the container.
  • Only a small number of molecules have very high velocity.
  • Between collisions, the molecules move in straight lines with constant velocities.
The compound A undergoes reaction as shown above.

Find out the reduction product of $$'A'$$.
128475_4cbe520cfb0447d6bd5962d1e0aa55b8.png
  • Isoamyl amine
  • Secondary butyl amine
  • Neopentyl amine
  • Tertiary amyl amine
A mixture of hydrogen and helium is prepared such that the number of wall collisions per unit time by molecules of each gas is the same. Which gas has the higher concentration?
  • Helium
  • Hydrogen
  • Both have same concentration
  • None of these
The gas constant has units:
  • $$L \: atm \: K^{-1} \: mol^{-1}$$
  • $$L \: atm^{-1} \: K^{-1} \: mol^{-1}$$
  • $$atm \:cm^3 \:K^{-1} \: mol^{-1}$$
  • $$erg\: K^{-1} $$
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 statements are true about the law of chemical combination?
  • Potassium combines with two isotopes of chlorine ($$^{35}Cl$$ and $$^{37}Cl$$) to form two samples of $$KCl$$. Their formation follows the law of definite composition.
  • Different proportions of oxygen in the various oxides of sulphur proves the law of multiple proportions.
  • $$H_2O$$ and $$H_2S$$ contain $$11.11\%$$ hydrogen and $$5.88\%$$ hydrogen respectively whereas $$SO_2$$ contains $$50\%$$ sulphur. The above data prove the law of reciprocal proportions.
  • In the decomposition of $$NH_3\ (2NH_3\xrightarrow {\Delta}N_2+3H_2)$$, the ratio of volumes of $$NH_3, N_2$$ and $$H_2$$ is $$2:1:3$$. The above data proves the Gay Lussac's law.
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
3000 cc of oxygen was burnt with 600 cc of ethane($$C_2H_6$$). Calculate the volume of unused oxygen.
  • 300 cc
  • 600 cc
  • 900 cc
  • 1200 cc
60 cc of oxygen was added to 24 cc of carbon monoxide and the mixture ignited. Calculate the volume of $$O_2$$ used up and the volume of $$CO_2$$ formed.
  • 15 cc, 30 cc
  • 12 cc, 24 cc
  • 20 cc, 40 cc
  • 10 cc, 20 cc
Which one of the following is the wrong statement about the liquid?
  • It has intermolecular force of attraction
  • Evaporation of liquids increases with the decrease of surface area
  • It resembles a gas near the critical temperature
  • It is an intermediate state between gaseous and solid state
At constant temperature, the pressure of a gas is __________ to its volume.
  • inversely proportional
  • directly proportional
  • not proportional
  • none of the above
For an ideal gas, number of mol per litre in terms of its pressure p, temperature T and gas constant R is:
  • p/RT
  • p/R
  • pT/R
  • RT/p
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
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
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
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
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
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:
  • $$0.33$$
  • $$0.2$$
  • $$0.25$$
  • $$0.52$$
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
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
An ideal gas is collected by downward displacement of water. Select the correct expression for $$P_{gas}$$ according to the diagram $$[d_{Hg} = 13.6 g/cm^3$$]:
698132_86cc151ecd164345adfa4fb6e8fdb720.png
  • $$P_{gas} = P_{atm} - \left[ aq.\ Tension + \dfrac{h}{13.6} \right]$$
  • $$P_{gas} = P_{atm} - hdg$$
  • $$P_{gas} = P_{atm} - aq.\ Tension + \dfrac{h}{13.6}$$
  • None of these.
The density of a liquid is 1.2 g/mL. That are 35 drops in 2 mL. The number of molecules in 1 drop is (molecular weight of liquid = 70): 
  • $$\frac{1.2}{35} N_A$$
  • $$\left (\frac{1}{35} N_A \right )^2$$
  • $$\frac{1.2}{(35)^2} N_A$$
  • $$1.2 N_A$$
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?
  • $$99.65\ g mol^{-1}$$
  • $$18 \ g mol^{-1}$$
  • $$134.1 \ g mol^{-1}$$
  • $$105.74\ g mol^{-1}$$
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%
$$18$$ g glucose ($$C_6H_{12}O_6$$) is added to $$178.2$$ g of water. The vapour pressure of this aqueous solution at $$100^0C$$ in torr is:
  • $$7.60$$
  • $$76.00$$
  • $$752.40$$
  • $$759.00$$
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
The reaction, $$ZnO(s)+CO(g) \rightleftharpoons  Zn(g)+{CO}_{2}(g)$$, has an equilibrium constant of $$1$$ atm at $$1500K$$. The equilibrium partial pressure of zinc vapour in a reaction vessel if an equimolar mixture of $$CO$$ and $${CO}_{2}$$ is brought into contact with solid $$ZnO$$ at $$1500K$$ and the equilibrium is achieved at $$1$$ atm is?
  • $$0.68$$ atm
  • $$0.76$$ atm
  • $$0.24$$ atm
  • $$0.5$$ atm
Vapour pressure of $$CCl_4$$ at $$25^0$$C is $$143$$mm Hg. $$0.5$$ gm of a non-volatile solute (mol.wt.$$65$$) is dissolved in $$100$$ ml of $$CCl_4$$. Find the vapour pressure of the solution. (Density of CCl_4 = $$1.58 gm/cm^3$$)
  • $$141.93$$mm
  • $$94.39$$mm
  • $$199.34$$mm
  • $$143.99$$mm
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