CBSE Questions for Class 11 Medical Chemistry States Of Matter Gases And Liquids Quiz 5 - MCQExams.com

An ideal gas undergoes a process in which $$T = T_{0} + aV^{3}$$, where $$T_{0}$$ and $$'a'$$ are positive constants and $$V$$ is molar volume. The molar volume for which pressure will be minimum is :
  • $$\left (\dfrac {T_{0}}{2a}\right )^{1/3}$$
  • $$\left (\dfrac {T_{0}}{3a}\right )^{1/3}$$
  • $$\left (\dfrac {a}{2T_{0}}\right )^{1/3}$$
  • None of these
A balloon contains $$14.0\ L$$ of air at $$760\ torr.$$. What will be the volume of the balloon when it is taken to a depth of $$10\ ft$$ in a swimming pool? Assume that the temperature of the air and water are equal (density: $$Hg=13.6\ g/mL$$)
  • $$11.0$$
  • $$11.3$$
  • $$10$$
  • $$10.8$$
The vapour pressure of a solvent decreased by $$10\ mm$$ of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is $$0.2$$. What should be the mole fraction of the solvent, if the decrease in the vapour pressure is to be $$20\ mm$$ of mercury?
  • $$0.8$$
  • $$0.6$$
  • $$0.4$$
  • $$0.2$$
If the mean free-path of gaseous molecule if 60 cm at a pressure of $$1\times 10^{-4}mm$$ mercury what will be its mean free-path when the pressure is increased to $$ 1\times 10^{-2}$$ mm mercury.
  • $$ .0 \times 10^{-1} cm$$
  • 0.6 cm
  • $$ .0 \times 10^{-2} cm$$
  • $$ .0 \times 10^{3} cm$$
Which of the following mixtures of gases does not obey Dalton's law of partial pressure?
  • $$O_{2}$$ and $$CO_{2}$$
  • $$N_{2}$$ and $$O_{2}$$
  • $$Cl_{2}$$ and $$O_{2}$$
  • $$NH_{3}$$ and $$HCl$$
Which mixture of gases at room temp does not obey daltons law of partial pressure?
  • $$He + Ne + O_{2}$$
  • $$CO_{2} + N_{2} + O_{2}$$
  • $$NH_{3} + HCl + O_{2}$$
  • $$N_{2} + O_{2} + CH_{4}$$
If K.E. of an electron, $$\alpha-particle$$ and a proton are represented by $$E_{1}, E_{2}$$ and $$E_{3}$$ respectively (provided all these have same de Broglie wavelength) then______________.
  • $$E_{1} = E_{2} = E_{3}$$
  • $$E_{1} > E_{2} > E_{3}$$
  • $$E_{1} > E_{3} > E_{2}$$
  • $$E_{2} > E_{3} > E_{1}$$
A open ended mercury manometer is used to measure the pressure exerted by a trapped gas as shown in the figure. Initially manometer shows no difference in mercury level in both columns as shown in figure.
After sparking $$A$$ dissociates according to following reaction 
$$A(g)\longrightarrow B(g)+3C(g)$$
If pressure of Gas $$A$$ decreases to $$0.9atm$$. Then
(Assume temperature to be constant and is $$300K$$)
781062_7be9bc1616374a2a98da1093a8638463.PNG
  • total pressure increased to $$1.3$$ atm
  • total pressure increased by $$0.3$$ atm
  • total pressure increased by $$22.3cm$$ of $$Hg$$
  • difference in mercury level is $$228mm$$
If the pressure of gas contained in a closed vessel is increased by 0.4% when heated by 1 degree C its initial temperature must be _____
  • $$20K$$
  • $$250K$$
  • $$25^oC$$
  • $$300K$$
The blotting paper absorbs liquids because
  • It has got small pores.
  • It is white.
  • An absorbing chemical is mixed.
  • None of these.
Which one of the following gases is lighter than air?
  • Carbon dioxide
  • Chlorine
  • Oxygen
  • Hydrogen
The $$K_p$$ for $$2SO_{2(g)+O_{2(g)}}\rightleftharpoons 2SO_{3(g)}$$ is $$5.0\,atm^{-1}$$.What is the equilibrium partial pressure of $$O_2$$ if the equilibrium pressure of $$SO_2$$ and $$SO_3$$ are equal?
  • 0.2
  • 0.3
  • 0.4
  • 0.1
At same temperature $$N_{2}O_{4}$$ is dissociated to $$40$$% and $$50$$% at total pressure $$P_{1}$$ and $$P_{2}$$ atm respectively in $$NO_{2}$$. Then the ratio of $$P_{1}$$ and $$P_{2}$$ is?
  • $$\dfrac {4}{5}$$
  • $$\dfrac {7}{4}$$
  • $$\dfrac {4}{7}$$
  • None of these
The property utilized in the manufacture of lead shots is
  • Specific weight of liquid lead
  • Specific gravity of liquid lead
  • Compressibility of liquid lead
  • Surface tension of liquid lead
The given diagram shows percentage composition of gases $$P, Q, R$$ and other gases present in air.
Which of the following statements is/ are correct regarding gases $$P, Q$$ and $$R$$?
(i) $$P$$ can be fixed in soil by certain bacteria present in roots of leguminous plants.
(ii) $$P$$ supports combustion whereas $$Q$$ and $$R$$ help in extinguishing fire.
(iii) Plants and animals release $$R$$ in respiration whereas plants use $$Q$$ in photosynthesis.
(iv) $$R$$ entraps sun's heat and makes earth warm and hospitable.
811494_4daa3bf34c9c48ccaa741604de5fbb65.jpg
  • (i) and (iv) only
  • (ii) and (iii) only
  • (i), (ii) and (iv) only
  • (iii) only
The molecular weights of $$O_2$$ and $$N_2$$ are $$32$$ and $$28$$ respectively. At $$15^0$$C, the pressure of $$1$$gm $$O_2$$ will be the same as that of $$1$$ gm $$N_2$$ in the same bottle at the temperature:
  • $$-21^0$$C
  • $$-13^0$$C
  • $$15^0$$C
  • $$56.4^0$$V
Lowering of vapour pressure in $$2$$ molal aqueous solution at $$373K$$ is____________.
  • $$0.35$$ bar
  • $$0.022$$ bar
  • $$0.22$$ bar
  • $$0.035$$ bar
For the reaction
$$A(g)+B(g)\rightleftharpoons C(g)$$, the equilibrium partial pressures are $${P}_{A}=0.15atm$$, $${P}_{B}=0.10atm$$ and $${P}_{C}=0.30atm$$. The value of the pressure was so reduced that after attainment of equilibrium again, the partial pressures of $$A$$ and $$B$$ were doubled. The partial pressure of $$C$$ would be:
  • $$0.30atm$$
  • $$0.60atm$$
  • $$1.20atm$$
  • $$1.80atm$$
With regard to the gaseous state of matter which of the following statements are correct?
  • Complete order of molecules
  • Complete disorder of molecules
  • Random motion of molecules
  • Fixed position of molecules
The rms speed of hydrogen is $$\sqrt { 7 }$$ times the rms speed of nitrogen. If T is the temperature of the gas, then:
  • $${ T }_{ { H }_{ 2 } }={ T }_{ { N }_{ 2 } }$$
  • $${ T }_{ { H }_{ 2 } }>{ T }_{ { N }_{ 2 } }$$
  • $${ T }_{ { H }_{ 2 } }<{ T }_{ { N }_{ 2 } }$$
  • $${ T }_{ { H }_{ 2 } }={ \sqrt { 7 } T }_{ { N }_{ 2 } }$$
The ratio of the vapour pressure of a solution to the vapour pressure of the solvent is:
  • equal to the mole fraction of the solvent
  • equal to the mole fraction of the solute
  • directly proportional to mole fraction of the solute
  • None of the above
At a given temperature, total vapour pressure in Torr of a mixture volatile components A and B is given by 
$$P_{Total}=120-75X_B$$
Hence, vapour pressure of pure A and B respectively (in Torr) are ?
  • 120, 75
  • 120, 195
  • 120, 45
  • 75, 45
Pressure exerted by one mole of an ideal gas kept in vessel of '$$V$$' L having root mean square molecule '$$V$$' and '$$m$$' mass of each molecule is correctly given by the equation?
  • $$P =$$ $$\dfrac {1}{2}$$$$\dfrac {N}{V}$$mv$$^{2}$$
  • $$P =$$ $$\dfrac {1}{3}$$$$\dfrac {N}{V}$$mv$$^{2}$$
  • $$P =$$ $$\dfrac {2}{3}$$$$\dfrac {N}{V}$$mv$$^{2}$$
  • $$P =$$ $$\dfrac {3}{2}$$$$\dfrac {N}{V}$$mv$$^{2}$$
Water and chlorobenzene are immiscible liquids. Their mixture boils at $$89^o$$C under a reduced pressure of $$7.7 \times 10^4$$ Pa. The vapour pressure of pure water at $$89^o$$C is $$7 \times 10^4$$ Pa. Weight percent of chlorobenzene in the distillate is:
  • 50
  • 60
  • 79
  • 38.46
Two glass bulbs A and B are connected by a very small tube having a stop cock. Bulb A has a volume of 100 $$cm^{3}$$ and contained the gas, while bulb B was empty. On opening the stop cock, the pressure fell down 40%. The volume of the bulb B must be ?
  • 75 $$cm^{3}$$
  • 125 $$cm^{3}$$
  • 150 $$cm^{3}$$
  • 250 $$cm^{3}$$
A pre-weighed vessel was filled with $$O_{2}$$ at STP and weighed. It was then evacuated, filled with $$SO_{2}$$ at the same temperature and pressure and again weighed. The weight of $$O_{2}$$ will be $$[O = 16, S = 32]$$.
  • The same as that of the $$SO_{2}$$
  • Twice as that of the $$SO_{2}$$
  • Half of that of the $$SO_{2}$$
  • One-fourth of that of the $$SO_{2}$$
At $$80^0$$C, the vapour pressure of pure liquid A is $$250$$mm of Hg and that of pure liquid B is $$1000$$ mm of Hg. If a solution of A and B boils at $$80^0$$C and $$1$$ atm pressure, the amount of A in the mixture is :$$(1atm = 760mm$$Hg)
  • $$50$$ mole percent
  • $$52$$ mole percent
  • $$32$$ mole percent
  • $$48$$ mole percent
Which of the following statement is wrong ? 
878683_1ab905a0db19439998016d0055cc5685.png
  • For gas A, a= 0 and z will linearly depend on pressure
  • For gas B, b = 0 and z will linearly depend on pressure
  • Gas C is real gas and we can find "a" and 'b' if intersection data is given
  • All vander waal gases will behave like gas C and give positive slope at high pressure
At $$80^o$$C, the vapour pressure of pure liquid $$A$$ is $$250$$ mm of $$Hg$$ and that of pure liquid $$B$$ is $$1000$$ mm of $$Hg$$. If a solution of $$A$$ and $$B$$ boils at $$80^o$$ and $$1$$ atm pressure, the amount of $$A$$ in the mixture is? 
($$1$$ atm $$=760$$ mm Hg).
  • $$50$$ mole percent
  • $$52$$ mole percent
  • $$32$$ mole percent
  • $$48$$ mole percent
The translational kinetic energy of an ideal gas depends only on its:
  • Pressure
  • Force
  • Temperature
  • Molar mass
On a humid day in summer, the mole fraction of gaseous $$H_{2}O$$ (water vapour) in the air at $$25^0$$C can be as high as $$0.0287$$. Assuming a total pressure of $$0.977$$ atm. What is the partial pressure of dry air?
  • $$94.9$$ atm
  • $$0.949$$ atm
  • $$949$$ atm
  • $$0.648$$ atm
Which of the following relationships for various gas laws is not correct?
  • $$V_{t} = V_{0} + \dfrac {V_{0}}{273}\times t$$
  • $$\dfrac {V_{1}}{T_{1}} = \dfrac {V_{2}}{T_{1}} (constant\ P)$$
  • $$\dfrac {P_{1}}{T_{1}} = \dfrac {P_{2}}{T_{1}} (constant\ V)$$
  • $$\dfrac {P_{1}T_{1}}{V_{1}} = \dfrac {P_{2}T_{2}}{V_{2}}$$
Two flasks of equal volume have been joined by a narrow tube of negligible volume. Initially, both flasks are at 300K containing 0.6 mole of $$O_2$$ at 0.5 atm pressure. one of the flasks is placed in the thermostat of 600K. FInd the number of mole of $$O_2$$ gas in each flask.
  • 0.5mol and 0.3 mol
  • 0.5mol and 0.2 mol
  • 0.4mol and 0.2 mol
  • 0.6mol and 0.3 mol
Which of the following values does not represent the correct value of $$R$$?
  • $$8.314\ Pa\ m^{2} K^{-1} mol^{-1}$$
  • $$8.314\times 10^{-2} bar\ L\ K^{-1} mol^{-1}$$
  • $$0.0821\ J\ K^{-1} mol^{-1}$$
  • $$8.314\ J\ K^{-1} mol^{-1}$$
The statements for laws of chemical combinations are given below. Mark the statement which is not correct.
  • Matter can neither be created nor destroyed: Law of conservation of mass
  • A compound always contains exactly the same proportion of elements by weight: Law of definite proportions
  • When gases combine they do so in a simple ratio by weight: Gay Lussac's Law
  • Equal volumes of gases at same temperature and pressure contain same number of molecules: Avogadro's Law
$$6 g$$. of the area of dissolved in $$90 g$$. of boiling water. The vapour pressure of the solution is: 
  • $$744.8$$ mm
  • $$758$$ mm
  • $$761$$ mm
  • $$760$$ mm
Which of the following statement about Avogadro's hypothesis is correct?
  • Under similar conditions of temperature and pressure, gases react with each other in simple ratio.
  • Under similar conditions of temperature and pressure, equal volumes of all gases contain same number of molecules
  • At NTP all gases contain same number of molecules
  • Gases always react with gases only at the given temperature and pressure
Two moles of pure liquid 'A' ($$P^o_A$$ = 80mm of Hg) and 3 moles of pure liquid 'B' ($$P^o_B$$ = $$120$$mm of $$Hg$$) are mixed. Assuming ideal behaviour.
  • Vapour pressure of the mixture is $$104$$ mm of $$Hg$$
  • Mole fraction of liquid '$$A'$$ in Vapour pressure is $$0.3077$$
  • Mole fraction of '$$B$$' in vapour pressure is $$0.692$$
  • Mole fraction of '$$B$$' in vapour pressure is $$0.785$$
At 80C, the vapour pressure of pure benzene is 753 mm Hg and of pure toluene 290 mm Hg. Calculate the composition of a liquid in mole percent which at $$80$$ is in equilibrium with vapour containing 30 mole percent of benzene. 
  • 24, 56
  • 26 ,54
  • 56 24
  • 34 ,76
To which of the following the Dalton's law of partial pressures is not applicable?
  • $$H_{2}$$ and $$He$$
  • $$NH_{3}$$ and $$HCl$$
  • $$N_{2}$$ and $$H_{2}$$
  • $$N_{2}$$ and $$O_{2}$$
A $$10\ L$$ flask contains a gaseous mixture of $$CO$$ and $$CO_{2}$$ at a total pressure of $$2\ atm$$ and $$298\ K$$. If $$0.20\ mole$$ of $$CO$$ is present, find its partial pressure.
  • $$0.49\ atm$$
  • $$1.51\ atm$$
  • $$1\ atm$$
  • $$2\ atm$$
How many number of moles of nitrogen will be present in $$2.24\ L$$ of nitrogen gas at $$STP?$$
  • $$9.9$$
  • $$0.099$$
  • $$0.001$$
  • $$1.00$$
Equal masses of helium and oxygen are mixed in a container at $$25^{\circ}C$$. The fraction of the total pressure exerted by oxygen in the mixture of gases is :
  • $$1/3$$
  • $$2/3$$
  • $$1/9$$
  • $$4/9$$
A gas occupies a volume of $$300\ cm^{3}$$ at $$27^{\circ}C$$ and $$620\ mm$$ pressure. The volume of gas at $$47^{\circ}C$$ and $$640\ mm$$ pressure is:
  • $$260\ cm^{3}$$
  • $$310\ cm^{3}$$
  • $$390\ cm^{3}$$
  • $$450\ cm^{3}$$
A closed container contains equal number of moles of two gases $$X$$ and $$Y$$ at a total pressure of $$710\ mm$$ of $$Hg$$. If gas $$X$$ is removed from the mixture, the pressure will :
  • become double
  • become half
  • remain same
  • become one-fourth
What will be the volume of $$2.8\ g$$ of carbon monoxide at $$27^{\circ}C$$ and $$0.821$$ atmospheric pressure?
  • $$2.5\ L$$
  • $$4\ L$$
  • $$3.5\ L$$
  • $$3\ L$$
Density of a gas is found to be $$5.46\ g/ dm^{3}$$ at $$27^{\circ}C$$ and $$2\ bar$$ pressure. What will be its density at STP?
  • $$3.0\ g\ dm^{-3}$$
  • $$5.0\ g\ dm^{-3}$$
  • $$6.0\ g\ dm^{-3}$$
  • $$10.82\ g\ dm^{-3}$$
What volume in litres will be occupied by $$4.4$$ g of $$CO_2$$ at STP?
  • $$22.4\ L$$
  • $$44.8\ L$$
  • $$12.2\ L$$
  • $$2.24\ L$$
What will be the pressure of the gas mixture of $$3.2\ g$$ methane and $$4.4\ g$$ carbon dioxide contained in at $$9\ dm^{3}$$ flask at $$27^{\circ}C$$?
  • $$0.82\ atm$$
  • $$8.314\times 10^{4}\ atm$$
  • $$1\ atm$$
  • $$1.8\ atm$$
$$34.05\ mL$$ of phosphorus vapours weight $$0.0625\ g$$ at $$546^{\circ}C$$ and $$0.1\ bar$$ pressure. What is the molar mass of phosphorus?
  • $$124.77\ g\ mol^{-1}$$
  • $$1247.74\ g\ mol^{-1}$$
  • $$12.47\ g\ mol^{-1}$$
  • $$30\ g\ mol^{-1}$$
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