MCQ Questions for Class 11 Engineering Chemistry States Of Matter Quiz 1

Which of the following law is followed by ideal gases?

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Charle's law
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Boyle's law
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Avogadro's law
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All of the above

A spherical balloon of

$21\ cm$ diameter is to be filled up with

$H_2$ at

$NTP$ from a cylinder containing the gas at

$20\ atm$ at

$27^{\circ}C$ . The cylinder can hold

$2.82$ litre of water. The number of balloons that can be filled up

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11
0%
10
0%
8
0%
1

Total pressure of a gaseous mix is equal to the sum of the Partial Pressures is:

0%
Boyle's law
0%
Charles's law
0%
Avogadro's principle
0%
Dalton's law

Which of the following is not an assumption of the kinetic theory of gases?

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Collision of gas particles are perfectly elastic.
0%
Gas particles have negligible volume.
0%
At high pressure, gas particles are difficult to compress.
0%
A gas consists of many identical particles which are in continual motion.

Which term describes the mass of

$6.022\times { 10 }^{ 23 }$ representative particles?

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Molar mass
0%
Avogadro's number
0%
Empirical formula
0%
Molecular formula

Explanation

Molar mass of a compound describes the total mass of

$6.023 \times 10^{23}$ atoms or particles of the compound.

Ex: Molar mass of

$H_2 = 2\space g$

Liquid

$M$ and liquid

$N$ form an ideal solution. The vapour pressures of pure liquids

$M$ and

$N$ are

$450$ and

$700\ mm$

$Hg$ , respectively, at the same temperature. Then correct statement is:
(

${x}_{M}=$ Mole fraction of

$M$ in solution;

${x}_{N}=$ Mole fraction of

$N$ in solution;

${y}_{M}=$ Mole fraction of

$M$ in vapour phase;

${y}_{N}=$ Mole fraction of

$N$ in vapour phase)

0%
$({x}_{M}-{y}_{M})< ({x}_{N}-{y}_{N})$
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$\cfrac{{x}_{M}}{{x}_{N}}< \cfrac{{y}_{M}}{{y}_{N}}$
0%
$\cfrac{{x}_{M}}{{x}_{N}}> \cfrac{{y}_{M}}{{y}_{N}}$
0%
$\cfrac{{x}_{M}}{{x}_{N}}= \cfrac{{y}_{M}}{{y}_{N}}$

Explanation

Since

$P^o_N>P^o_M,$ so

$N$ is more volatile than

$M.$

$\therefore y_N>x_N$

and

$x_M>y_M$

Multiply we get

$y_N\times x_M>x_N \times y_M$

$i.e.\ \dfrac{x_M}{x_N}=\dfrac{y_M}{y_N}$

When an ideal gas undergoes unrestrained expansion, no cooling occurs because the molecules :

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Are above the inversion temperature
0%
Exert no attractive forces on each other
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Do work equal to loss in kinetic energy
0%
Collide without losing energy

According to kinetic theory of gases :

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collisions are always elastic
0%
heavier molecules transfer more momentum to the wall of the container
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only a small number of molecules have very high velocity
0%
between collisions, the molecules move in straight lines with constant velocities

The correction factor

$'a'$ to the ideal gas equation corresponds to:

0%
electric field present between the gas molecules
0%
density of the gas molecules
0%
forces of attraction between the gas molecules
0%
volume of the gas molecules

Explanation

The correction factor

$'a'$ to the ideal gas equation corresponds to forces of attraction between the gas molecules. Greater the value of

$'a'$ , more easily a gas can be liquefied. The unit of

$'a'$ is

$atm L^{2}mol^{-2}$ .

Gay Lussac's law of gaseous volume is derived from :

0%
law of definite proportions
0%
law of multiple proportions
0%
law of reciprocal proportions
0%
experimental observation

Statement I: Hydrogen gas

$(H_{2})$ is considered a perfectly ideal gas.

Statement II: Hydrogen atoms interact with each other via hydrogen bonds.

When statement is true then T and otherwise F.

0%
F, F
0%
TT
0%
TF
0%
FT

Explanation

Statement-1: The gas which has zero intermolecular forces and zero molecular volume is considered a perfect ideal gas. In the case of hydrogen, the conditions for an ideal gas are not satisfied. Therefore,

$H_2$ gas is not a perfectly ideal gas.

Statement-2: The hydrogen bond is formed between a less electronegative hydrogen atom and more electronegative

$O, N$ , and

$F$ atoms. Thus, hydrogen atoms do not interact with each other via hydrogen bonds.

Hence, both the given statements are false. So option A is correct.

At same temperature and pressure, equal volumes of gases contain the same number of:

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molecules
0%
electrons
0%
protons
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particles

The kinetic energy of a molecule of a gas is directly proportional to the absolute temperature of the gas.

0%
True
0%
False

$\dfrac{P_{1}V_{1}}{T_{1}} = \dfrac{P_{2}V_{2}}{T_{2}}$ is true for :

0%
Boyle's law
0%
Charle's law
0%
Ideal gas equation
0%
Combined gas law
0%
Dalton's law of partial pressures

Explanation

combined gas law equation.

The combined gas law is a gas law that combines Charles's law, Boyle's law, and Gay-Lussac's law. The ratio between the pressure-volume product and the temperature of a system remains constant. so question should be like P1V1T2 $=$ P2V2T1

At constant volume, pressure is directly proportional to the temperature, this law is popularly known as :

0%
Charle's law
0%
Boyle's law
0%
Gay Lussac law
0%
Avogadro law

Explanation

According to Gay Lussac's law, pressure is directly proportional to temperature at constant volume.

$P\propto T$

According to the Avogadro's Law, equal volumes of two different gases, under same conditions of temperature and pressure, contain equal number of:

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atoms
0%
molecules
0%
electrons
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protons

Equal volume of gases contain equal number of moles.

State whether the above statement is true or false.

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The statement is True
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The statement is False
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Neither
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Equal volume of gases contain equal number of moles, only when the temperature is increased

The graph pressure versus temperature

$(T)$ at constant volume is a straight line.

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True
0%
False

Avogadro's law finds an application in the determination of:

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Atomicity of gas
0%
Molecular weights of gases
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Molecular formula of certain gaseous compounds
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All the above

Gay Lussac law gives relation between:

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$P\,$ and $\,V$
0%
$P\,$ and $\,T$
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$V\,$ and $\,T$
0%
none of these

Which of the following statements is the most accurate with regard to the significance of Avogadro's number,

$6.02 \times 10^{23}$ ?

0%
It is the conversion factor between grams and atomic mass units.
0%
It is a universal physical constant just as the speed of light.
0%
It is the number of particles that is required to fill a $1\ L$ container.
0%
It is the inverse diameter of an $H$ atom .

Explanation

A carbon atom weighs 12 AMU, one AMU is equivalent to

$1.66 \times 10^{-24}$ grams. Conversely, one gram is equivalent to

$6.022 \times 10^{23}$ AMU, which is called Avogadro's number

so the answer is A

Which of the following solution in water will have the lowest vapour pressure?

0%
$0.1 M, NaCI$
0%
$0.1 M, Sucrose$
0%
$0.1 M,{ BaCI }_{ 2 }$
0%
$0.1 M { Na }_{ 3 }{ PO }_{ 4 }$

Explanation

$Na_3PO_4$ will give maximum ions in water (

$4$ ions)

So, it has lowest vapour pressure.

Which statement is linked with the idea that two identical containers filled with different gases will contain the same number of particles?

0%
Mosely
0%
Avagadro
0%
Dalton
0%
Mendeleev

${ \left( \cfrac { \partial H }{ \partial P } \right) }_{ T }$ for an ideal gas is equal to:

0%
zero
0%
$\cfrac { \Delta VRT }{ P }$
0%
$\cfrac { P\Delta V }{ T }$
0%
$nR\Delta T$

Which gas law should be used to solve a gas problem in which only the pressure and temperature of a gas change?

0%
Boyle's Law
0%
Ideal Gas Law
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Combined Gas Law
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Gay-Lussac's Law

All gases have the same number of moles in the same volume at constant temperature and pressure.

0%
Boyle's Law
0%
Charles's Law
0%
Avogadro's Principle
0%
Ideal Gas Law

Which of the following would have the lowest vapor pressure in the pure state?

0%
Sodium hydroxide because of the strong interparticle forces of ionic solids
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Methanol because of the hydrogen bonding in the functional group along with the non-polar nature of the carbon hydrogen bonds
0%
Water because of the very strong hydrogen bonding in the substances
0%
Ammonia because of the unbonded pair of electrons on the central atom coupled with hydrogen bonding in the substance.

Which gas can be collected over water?

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$NH_{3}$
0%
$N_{2}$
0%
$HCl$
0%
$SO_{2}$

Which of the following represents a combination of Boyle's Law and Charle's Law?

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$P_{1}V_{1}T_{1}= P_{2}V_{2}T_{2}$
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$\dfrac{P_{1}T_{2}}{V_{2}}=\dfrac{P_{2}T_{1}}{V_{1}}$
0%
$\dfrac{P_{1}T_{2}}{V_{1}}=\dfrac{P_{2}T_{1}}{V_{2}}$
0%
$\dfrac{T_{2}V_{1}}{P_{1}}=\dfrac{T_{1}V_{2}}{P_{2}}$

Explanation

Charles' law is the change in volume with respect to temperature at constant pressure, while Boyle's law is the change in volume with respect to pressure at a constant temperature.

Taking a gas of volume

$V_1$ , pressure

$P_1$ and temperature

$T_1$ , and let its change have a state (

$V_2, P_2, T_2$ ), then according to Boyle's law,

$P_1V_1=P_2V_2$ ..........(1)

Then keeping this constant pressure, move to state (

$V_2, P_2, T_2$ ) using Charles' law,

$\dfrac{V_1}{T_1}= \dfrac {V_2}{T_2}$ .........(2)

Solving for

$V_2$ , in both (1) and (2) and then equating them, we get-

$\dfrac {P_1V_1}{T_1} = \dfrac {P_2V_2}{T_2}$

After changing the pressure, volume and temperature of the gas, still their product is equal, suggesting that the relation is constant:

$\dfrac {PV}{T}=k$ .

Hence, the correct answer is option

$\text{B}$ .

In a given mixture of non-reacting gases, the ratio of partial pressure of each gas is equal to its:

0%
weight percent
0%
volume percent
0%
mole fraction
0%
critical pressure

The value of the universal gas constant

$R$ depends upon the:

0%
nature of the gas
0%
mass of the gas
0%
temperature of the gas
0%
units of measurement

Explanation

The value of the universal gas constant

$R$ depends on the units used for pressure, volume and temperature. Therefore, it depends on the units of measurement.

The pressure at which liquid and vapour can coexist at equilibrium is called the :

0%
limiting vapour pressure
0%
real vapour pressure
0%
normal vapour pressure
0%
saturated vapour pressure

$V$ versus

$T$ curves at constant pressure

$P_{1}$ and

$P_{2}$ for an ideal gas are shown in the figure given above. Choose the correct relation.

0%
$P_{1} > P_{2}$
0%
$P_{1} < P_{2}$
0%
$P_{1} = P_{2}$
0%
Cannot be related

Explanation

According to Charles's law, when the pressure on a sample of a dry gas is held constant, the Kelvin temperature and the volume will be directly related.

This directly proportional relationship can be written as:

$V \propto T$ &

$P \propto T$

For the above case, let us consider at a point volume is constant. We find that the temperature of the gas at pressure

$P_2$ is greater than that of gas at pressure

$P_1$ .

$\therefore$

$P_1 < P_2$

Hence, Option "B" is the correct answer.

Dalton's law of partial pressure is not applicable to which of the following mixture of gases?

0%
$H_{2}+F_{2}$
0%
$NH_{3}+HCl$
0%
$SO_{2}+Cl_{2}$
0%
$H_{2}+O_{2}$

Explanation

According to Dalton's law of partial pressures, for a mixture of non-reacting gases, the total pressure is equal to the sum of the partial pressures of the individual gases.

This law is not applicable to the mixtures

$H_{2}+F_{2}, NH_{3}+HCl$ and

$SO_{2}+Cl_{2}$ and

$H_{2}+O_{2}$ as they react with each other.

For example, hydrogen and fluorine react to form hydrogen fluoride.

0%
Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
0%
Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
0%
Assertion is correct but Reason is incorrect
0%
Assertion is incorrect but Reason is correct

Explanation

The volume ratio of

$H_{2} ,Cl_{2}$ and

$HCl$ in the reaction

$H_{2}+Cl_{2}\rightarrow 2HCl$ is

$1 : 1 : 2$ .

This is an example of Gay Lussac's law of combining volumes of gases which states that, "when gases react together to produce gaseous products, the volumes of reactants and products bear a simple whole-number ratio with each other, provided volumes are measured at same temperature and pressure ".

Thus, both Assertion and Reason are correct and Reason is the correct explanation for Assertion.

Hence, the correct answer is option

$\text{A}$ .

Which of the following is a correct representation for an ideal gas?

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$P_{1}d_{1}T_{1}=P_{2}d_{2}T_{2}$
0%
$\dfrac{d_{1}P_{1}}{T_{1}}=\dfrac{d_{2}P_{2}}{T_{2}}$
0%
$\dfrac{P_{1}}{d_{1}T_{1}}=\dfrac{P_{2}}{d_{2}T_{2}}$
0%
$\dfrac{P_{1}T_{1}}{d_{1}}=\dfrac{P_{2}T_{2}}{d_{2}}$

Explanation

$PV=nRT$

$PV=\dfrac{Mass}{Mol.\ wt}RT$

$P=\dfrac{Mass}{V}\dfrac{RT}{Mol.\ wt}$

$P=d\dfrac{RT}{Mol.\ wt}$

$d= \dfrac {PM} {RT}$

$\implies \dfrac{P_{1}}{d_{1}T_{1}}=\dfrac{P_{2}}{d_{2}T_{2}}$

For which of the following mixture of gases, Dalton's law of partial pressure is not applicable at room temperature?

0%
$HCl+NH_{3}$
0%
$CO+CO_{2}$
0%
$O_{2}+N_{2}$
0%
$SO_2+O_{2}$

Explanation

Dalton's law of partial pressure is not applicable at room temperature for a mixture of reacting gases.

Thus, Dalton's law of partial pressure is not applicable at room temperature for a mixture of (A) hydrogen chloride and ammonia.

Hence, the correct answer is option

$\text{A}$ .

The total pressure of a mixture of two gases is:

0%
the sum of the partial pressure
0%
the difference between the partial pressure
0%
the product of the partial pressure
0%
the ratio of the partial pressure

Which of the following mixture does not obey Dalton's law of partial pressures?

0%
$SO_{2}+Cl_{2}$
0%
$NH_{3}+PH_{3}$
0%
$CO_{2}+N_{2}$
0%
$CO+CO_{2}$

Explanation

$SO_{2}+Cl_{2}\rightarrow SO_2Cl_2$

$SO_{2}+Cl_{2}$ does not obey the Dalton's law of partial pressures because it is valid for non-reacting gases.

The value of gas constant in Joules/ K-mole is:

0%
8.314
0%
8.314 x 10 $^{7}$
0%
1.987
0%
0.0821

Explanation

According to ideal gas equation,

$PV=nRT$

P = Pressure, V = Volume, n = number of moles, T = Temperature, n = number of moles.

The value of a gas constant is 8.314 Joules/K-mole.

Which of the following indicates the value of gas constant?

0%
$1.987 cal \ K-mole$
0%
$8.3 cal \ deg \ mole$
0%
$0.0821 lit \ deg \ mole$
0%
$1.987\ Joules \ deg \ mole$

Explanation

In a gas equation

$PV = nRT$ the value of universal gas constant depends upon the units of measurement. Its values are

$\displaystyle 8.314 \: J/mol/K$ ,

$\displaystyle 0.0821 L.atm/mol/K$ ,

$\displaystyle 1.987 cal/mol/K$

When two molecules of an ideal gas collide:

0%
heat is liberated
0%
no heat is liberated
0%
heat is absorbed
0%
there is a decrease in the total K.E

According to kinetic theory of gases, there are:

0%
intermolecular attractions
0%
molecules have considerable volumes
0%
no intermolecular attractions
0%
velocity of molecules decreases for each collision

Which is wrong according to kinetic theory?

0%
The average kinetic energy of the molecules is directly proportional to the absolute temperature.
0%
All the molecules in a gas have the same kinetic energy.
0%
Collisions between molecules are perfectly elastic.
0%
Pressure is due to the impact of the molecules on the walls of the container.

Explanation

K.E. =

$\cfrac {1}{2} mv^2$ and from Maxwell distribution curve it can be seen that molecules of all the gases have a wide range of speed so they have different kinetic energy.

Hence option B is correct.

Which of the following values is not correct?

0%
$R = 8.314$ $JK$ $^{-1}$ $mol$ $^{-1}$
0%
$R = 62.36$ $torr$ $K$ $^{-1}$ $mol$ $^{-1}$
0%
$R = 0.0821$ $lit - atm$ $K$ $^{-1}$ $mol$ $^{-1}$
0%
$R = 2$ $cal$ $K$ $^{-1}$ $mol$ $^{-1}$

Explanation

The value of R (gas constant) has different values in different units.

$R = 8.314 \ J/K-mol$

$R = 62.36 \ torr/K-mol$

$R = 0.0821 \ L-atm/K-mol$

$R = 2 \ calories/K-mol$

When an ideal gas undergoes expansion through a porous plug, the gas is expected to exhibit no cooling because ___________.

0%
there exist no molecular forces of attraction
0%
the molecules collide with each other, without any loss of energy
0%
the volume occupied by molecules is negligible in comparision to the volume of the gas
0%
none of the above

Which is wrong according to kinetic theory of gases?

0%
Average $KE$ of molecules is proportional to the absolute temperature
0%
Collisions between molecules are perfectly elastic
0%
Pressure is due to collisions between molecules
0%
There are no attractive forces between the molecules of gas

In a 2.5

$L$ flask at

$27^{\circ}C$ temperature, the pressure of a gas was found to be 8

$atm$ . If

$2.41 \times 10^{23}$ molecules of the same gas are introduced into the container, the temperature changed to

$T_2$ . The pressure of gas is found to be 10

$atm$ . Find out the value of

$T_2$ :

0%
253 $K$
0%
347 $K$
0%
230 $K$
0%
370 $K$

Explanation

$6.023 \times 10^{23}$ molecules corresponds to 1

$mole$

$2.41 \times 10^{23}$ molecules corresponds to

$\displaystyle =\frac{2.41 \times 10^{23}}{6.023 \times 10^{23}}=0.4\ moles$
Case (i)

$P_1 V_1 = n_1 R_1 T_1$

$8(2.5)=n_1 (0.08) (300)$

$n_1 = \displaystyle \frac{8(2.5)}{(0.08)(300)}= 0.833\ moles$
Total moles

$n_2 = 0.833 +0.4$

$n_2 = 1.233$
Case (ii)

$P_2V_2=n_2R T_2$

$10(2.5)=1.233 (0.08) T_2$

$T_2=253.4$

Kinetic energy of molecules is highest in:

0%
gases
0%
solids
0%
liquids
0%
solutions

Which of the following is a representation of Gay-Lussac's law?

0%
$P_{1}T_{1}=P_{2}T_{2}$
0%
$P_{1}T_{2}=P_{2}T_{1}$
0%
$P_{1}V_{1}=P_{2}V_{2}$
0%
$V_{1}T_{2}=V_{2}T_{1}$

Explanation

According to Gay-Lussac's law, at constant volume, the pressure of the gas is proportional to it's absolute temperature.

So,

$\dfrac{P_{1}}{T_{1}} = \dfrac{P_{2}}{T_{2}}$

This gives,

$P_{1}T_{2} = P_{2}T_{1}$ .

CBSE Questions for Class 11 Engineering Chemistry States Of Matter Quiz 1 - MCQExams.com

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Practice Class 11 Engineering Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Engineering Chemistry States Of Matter Quiz 1 - MCQExams.com

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Practice Class 11 Engineering Chemistry Quiz Questions and Answers

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