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States of Matter Chemistry - States of Matter

MP Board (MPBSE) - STD 11 Science - Chemistry (Madhya Pradesh - English Medium). 342 questions in this chapter.

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States of Matter question types

342 questions across 7 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

342
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7
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5
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Sample Questions

States of Matter questions

One sample from each question group in this chapter. Select any group above to see the full set with answer keys.

Q 1M.C.Q (1 Marks)1 Mark
According to kinetic theory of gases :
  • A
    Collisions are always elastic
  • ✓
    Heavier molecules transfer more momentum to the wall of the container
  • C
    Only a small number of molecules have very high velocity
  • D
    Only a small number of molecules have very high velocity

Answer: B.

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Q 2M.C.Q (1 Marks)1 Mark
The certain volume of a gas exerts on its walls some pressure at a particular temperature. It has been found that by reducing the volume of the gas to half of its original value the pressure becomes twice that of the initial value at a constant temperature. This happens because :
  • A
    mass of the gas increases with pressure
  • B
    speed of the gas molecules decreases
  • ✓
    more number of gas molecules strikes the surface per second
  • D
    more number of gas molecules strikes the surface per second

Answer: C.

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Q 3M.C.Q (1 Marks)1 Mark
The total pressure of a gaseous mixture is equalto the sum of the partial pressures is:
  • A
    Boyles law
  • B
    Charles law
  • C
    Ideal gas law
  • ✓
    Daltons law

Answer: D.

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Q 5M.C.Q (1 Marks)1 Mark
The pressure exerted by the gaseous molecules is due to :
  • A
    The repulsion between gaseous molecules.
  • B
    The attraction between gaseous molecules.
  • ✓
    Collision of the particles with the walls of the container.
  • D
    Collision of the particles with the walls of the container.

Answer: C.

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Q 6Assertion (A) & Reason (B) MCQ1 Mark
Assertion $(A)$ : The temperature at which vapour pressure of a liquid is equal to the external pressure is called boiling temperature.
Reason $(R)$ : At high altitude atmospheric pressure is high.
  • A
    $A$ and $R$ both are correct, and $R$ is the correct explanation of $A.$
  • B
    $A$ and $R$ both are correct, but $R$ is not the correct explanation of $A$.
  • ✓
    $A$ is true but $R$ is false.
  • D
    $A$ and $R$ both are false.

Answer: C.

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Q 7Assertion (A) & Reason (B) MCQ1 Mark
Assertion $(A)$ : Gases do not liquefy above their critical temperature, even on applying high pressure.
Reason $(R)$ : Above critical temperature, the molecular speed is high and intermolecular attractions cannot hold the molecules together because they escape because of high speed.
  • ✓
    $A$ and $R$ both are correct, and $R$ is the correct explanation of $A.$
  • B
    $A$ and $R$ both are correct, but $R$ is not the correct explanation of $A$.
  • C
    $A$ is true but $R$ is false.
  • D
    $A$ and $R$ both are false.

Answer: A.

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Q 8Assertion (A) & Reason (B) MCQ1 Mark
In the following questions a statement of Assertion $(A)$ followed by a statement of Reason $(R)$ is given. Choose the correct option out of the choices given below each question. $44.$
Assertion $(A)$ : Three states of matter are the result of balance between intermolecular forces and thermal energy of the molecules.
Reason $(R)$ : Intermolecular forces tend to keep the molecules together but thermal energy of molecules tends to keep them apart.
  • ✓
    $A$ and $R$ both are correct, and $R$ is the correct explanation of $A.$
  • B
    $A$ and $R$ both are correct, but $R$ is not the correct explanation of $A$.
  • C
    $A$ is true but $R$ is false.
  • D
    $A$ and $R$ both are false.

Answer: A.

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Q 9Assertion (A) & Reason (B) MCQ1 Mark
Assertion $(A)$ : At critical temperature liquid passes into gaseous state imperceptibly and continuously.
Reason $(R)$ : The density of liquid and gaseous phase is equal to critical temperature.
  • ✓
    $A$ and $R$ both are correct, and $R$ is the correct explanation of $A.$
  • B
    $A$ and $R$ both are correct, but $R$ is not the correct explanation of $A$.
  • C
    $A$ is true but $R$ is false.
  • D
    $A$ and $R$ both are false.

Answer: A.

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Q 10Assertion (A) & Reason (B) MCQ1 Mark
Assertion $(A)$ : At constant temperature, $pV$ vs $V$ plot for real gases is not a straight line.
Reason $(R)$ : At high pressure all gases have $Z > 1$ but at intermediate pressure most gases have $Z < 1.$
  • ✓
    $A$ and $R$ both are correct, and $R$ is the correct explanation of $A.$
  • B
    $A$ and $R$ both are correct, but $R$ is not the correct explanation of $A$.
  • C
    $A$ is true but $R$ is false.
  • D
    $A$ and $R$ both are false.

Answer: A.

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Q 121 Marks Question1 Mark
The van der Waals' constants for two gases are as follows:
Gas a$\left(\operatorname{atm} \mathrm{L}^2 \mathrm{~mol}^{-2}\right)$ b$\left(\mathrm{L} \mathrm{~mol}^{-1}\right)$
X 1.39 0.0391
Y 3.059 0.0427
Which of them is more easily liquefiable and which has greater molecular size?
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Q 162 Marks Questions2 Marks
Critical temperature for carbon dioxide and methane are 31.1°C and –81.9°C respectively. Which of these has stronger intermolecular forces and why?
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Q 192 Marks Questions2 Marks
Two different gases ‘A’ and ‘B’ are filled in separate containers of equal capacity under the same conditions of temperature and pressure. On increasing the pressure slightly the gas ‘A’ liquefies but gas B does not liquify even on applying high pressure until it is cooled. Explain this phenomenon.
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Q 233 Marks Question3 Marks
Calculate the volume occupied by $8.8 \mathrm{~g}$ of $\mathrm{CO}_2$ at $31.1^{\circ} \mathrm{C}$ and 1 bar pressure. $\mathrm{R}=0.083$ bar $\mathrm{LK}^{-1} \mathrm{~mol}^{-1}$.
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Q 253 Marks Question3 Marks
A mixture of CO and $CO_2$ is found to have a density of $1.50gL^{-1}$ at 20°C and 740mm pressure. Calculate the composition of the mixture.
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Q 26Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions from (i) to (v).
Chemical properties of a substance do not change withthe change of its physical state; but rate of chemicalreactions do depend upon the physical state. Many timesin calculations while dealing with data of experiments werequire knowledge of the state of matter. Therefore, itbecomes necessary for a chemist to know the physical laws which govern the behaviour of matter indifferent states. Intermolecular forces are the forces ofattraction and repulsion between interactingparticles (atoms and molecules). This termdoes not include the electrostatic forces thatexist between the two oppositely charged ionsand the forces that hold atoms of a moleculetogether i.e., covalent bonds.Attractive intermolecular forces are knownas van der Waals forces, in honour of Dutchscientist Johannes van der Waals (1837-1923) . van der Waals forces vary considerablyin magnitude and include dispersion forcesor London forces, dipole-dipole forces, anddipole-induced dipole forces. A particularlystrong type of dipole-dipole interaction ishydrogen bonding. Only a few elements canparticipate in hydrogen bond formation, therefore it is treated as a separatecategory.
Atoms and nonpolar molecules are electricallysymmetrical and have no dipole momentbecause their electronic charge cloud issymmetrically distributed. But a dipole maydevelop momentarily even in such atoms andmolecules. The temporary dipoles of two different atomattract each other. Similarly temporary dipolesare induced in molecules also. This force ofattraction was first proposed by the Germanphysicist Fritz London, and for this reasonforce of attraction between two temporary dipoles is known as London force. dispersion force forces are always attractive and interactionenergy is inversely proportional to the sixthpower of the distance between two interactingparticles (i.e.,$1/r ^6$ where r is the distancebetween two particles). These forces areimportant only at short distances (~500 pm)and their magnitude depends on thepolarisability of the particle.
Dipole-dipole forces act between the moleculespossessing permanent dipole. Ends of thedipoles possess “partial charges” and thesecharges are shown by Greek letter delta (δ).Partial charges are always less than the unitelectronic charge $(1.6\times 10^{–19} C)$. The polarmolecules interact with neighbouringmolecules. This interactionis stronger than the London forces but isweaker than ion-ion interaction because onlypartial charges are involved. The attractiveforce decreases with the increase of distancebetween the dipoles. As in the above case herealso, the interaction energy is inverselyproportional to distance between polarmolecules. Dipole-dipole interaction energybetween stationary polar molecules is proportional to $1/r^3$ and thatbetween rotating polar molecules is proportional to $1/r ^6$​​​​​​​, where r is the distancebetween polar molecules.
Dipole–Induced Dipole Forcesare type of attractive forces operate betweenthe polar molecules having permanent dipoleand the molecules lacking permanent dipole.Permanent dipole of the polar moleculeinduces dipole on the electrically neutralmolecule by deforming its electronic cloud. Thus an induced dipole is developedin the other molecule. In this case alsointeraction energy is proportional to $1/r ^6$​​​​​​​​​​​​​​ where r is the distance between twomolecules. Induced dipole moment dependsupon the dipole moment present in thepermanent dipole and the polarisability of theelectrically neutral molecule.
  1. Partial charges are always less than the unit electronic charge:
  1. $(1.6\times 10^{–19} C)$
  2. $(1.6\times 10^{–18} C)$
  3. $(1.6\times 10^{–17}C)$
  4. $(1.6\times 10^{–16} C)$
  1. Temporary dipoles are induced in molecules also. ,this force of attraction was first proposed by:
  1. Johannes van der Waals
  2. Fritz London
  3. Robert Boyle
  4. Joseph Lewis Gay Lussac
  1. Atoms and nonpolar molecules are electrically:
  1. Compositional
  2. Unsymmetrical
  3. Symmetrical
  4. All the above
  1. Partial Charges denoted by greek letter ….
  1. $\in$
  2. $\zeta$
  3. $\delta$
  4. $\eta$
  1. The attractive force … with the … of distance between the dipoles.
  1. Increase, increase
  2. Decrease, decrease
  3. Increase, decrease
  4. Decreases, increase
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Q 27Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions from (i) to (v).
It is well known fact that liquids assume theshape of the container. Why is it then smalldrops of mercury form spherical bead insteadof spreading on the surface. Why do particlesof soil at the bottom of river remain separatedbut they stick together when taken out? Whydoes a liquid rise (or fall) in a thin capillary assoon as the capillary touches the surface ofthe liquid? All these phenomena are causeddue to the characteristic property of liquids,called surface tension. A molecule in the bulkof liquid experiences equal intermolecularforces from all sides. The molecule, thereforedoes not experience any net force. But for themolecule on the surface of liquid, net attractiveforce is towards the interior of the liquid, due to the molecules below it. Since thereare no molecules above it.Liquids tend to minimize their surface area.The molecules on the surface experience a netdownward force and have more energy than the molecules in the bulk, which do notexperience any net force. Therefore, liquids tendto have minimum number of molecules at theirsurface. If surface of the liquid is increased bypulling a molecule from the bulk, attractiveforces will have to be overcome. This willrequire expenditure of energy. The energyrequired to increase the surface area of theliquid by one unit is defined as surface energy.Its dimensions are Jm. Surface tension isdefined as the force acting per unit lengthperpendicular to the line drawn on the surfaceof liquid. It is denoted by Greek letter γ(Gamma). It has dimensions of kg $s^{–2}$ and in SIunit it is expressed as $Nm^{–1}.$
The lowest energystate of the liquid will be when surface area isminimum. Liquid tends to rise (or fall) in the capillarybecause of surface tension. Liquids wet thethings because they spread across their surfacesas thin film. Moist soil grains are pulled togetherbecause surface area of thin film of water isreduced. It is surface tension which givesstretching property to the surface of a liquid.On flat surface, droplets are slightly flattenedby the effect of gravity; but in the gravity freeenvironments drops are perfectly spherical. Viscosity is a measure of resistance toflow which arises due to the internal frictionbetween layers of fluid as they slip past oneanother while liquid flows. Strongintermolecular forces between molecules holdthem together and resist movement of layerspast one another.
When a liquid flows over a fixed surface,the layer of molecules in the immediate contactof surface is stationary. The velocity of upperlayers increases as the distance of layers fromthe fixed layer increases. This type of flow inwhich there is a regular gradation of velocityin passing from one layer to the next is calledlaminar flow.‘$ η’$ is proportionality constant and is calledcoefficient of viscosity. Viscosity coefficientis the force when velocity gradient is unity andthe area of contact is unit area. Thus ‘$ η’$ ismeasure of viscosity. SI unit of viscositycoefficient is $1$ newton second per square metre $\left( N s m ^{-2}\right)=$ pascal second (Pa s $\left.=1 g cm ^{-1} s^{-1}\right)$. Incgs system the unit of coefficient of viscosity ispoise (named after great scientist Jean LouisePoiseuille). 1 poise $=1 g cm ^{-1} S^{-1}=10^{-1} kg m ^{-1} S^{-1}$ Greater the viscosity, the more slowly theliquid flows. Hydrogen bonding and van derWaals forces are strong enough to cause highviscosity. Glass is an extremely viscous liquid.It is so viscous that many of its propertiesresemble solids.Viscosity of liquids decreases as thetemperature rises because at high temperaturemolecules have high kinetic energy and canovercome the intermolecular forces to slip pastone another between the layers.
  1. The dimension of surface energy is:
  1. $Jm^{–2}$
  2. $Jm^2$
  3. $Kjm^{–2}$
  4. $Kjm^2$
  1. 1 poise =
  1. $1cmskg^{-1}$
  2. $1gcm^{–1}s^{–1}$
  3. $1gcms^–1$
  4. $1gcm^{–1}s$
  1. Which of the following is most viscous liquid?
  1. Glass
  2. Water
  3. Mercury
  4. Kerosene
  1. Surface Tension denoteed by greek letter...
  1. $\in$
  2. $\zeta$
  3. $\delta$
  4. $\gamma$
  1. Flow in which there is a regular gradation of velocity in passing from one layer to the next is called:
  1. Turbulent flow
  2. Shear flow
  3. Streamline flow
  4. laminar flow.
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Q 28Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions from (i) to (v).
First complete data on pressure-volume-Temperature relations of a substance in bothGaseous and liquid state was obtained byThomas Andrews on Carbon dioxide. He plottedlsotherms of carbon dioxide at variousTemperatures.
Later on it was found That real gases behave in the same manner asCarbon dioxide. Andrews noticed that at highTemperatures isotherms look like that of anldeal gas and the gas cannot be liquified even atVery high pressure. As the temperature isLowered, shape of the curve changes and dataShow considerable deviation from idealBehaviour. At $30.98^{\circ} C$ carbon dioxide remainsGas upto 73 atmospheric pressure. At 73 atmospheric pressure, liquidCarbon dioxide appears for the first time. TheTemperature $30.98^{\circ} C$ is called criticalTemperature (TC) of carbon dioxide. This is theHighest temperature at which liquid carbonDioxide is observed. Above this temperature itls gas. Volume of one mole of the gas at criticalTemperature is called critical volume $\left( V _{ c }\right)$ andPressure at this temperature is called criticalPressure (pc). The critical temperature, pressureand volume are called critical constants. A gasBelow the critical temperature can be liquifiedBy applying pressure, and is called vapour ofThe substance. Carbon dioxide gas below itsCritical temperature is called carbon dioxideVapour.
Intermolecular forces are stronger in liquidState than in gaseous state. Molecules in liquidsAre so close that there is very little empty space between them and under normal conditionsLiquids are denser than gases.Molecules of liquids are held together byAttractive intermolecular forces. Liquids haveDefinite volume because molecules do notSeparate from each other. However, moleculesOf liquids can move past one another freely, Therefore, liquids can flow, can be poured andCan assume the shape of the container in whichThese are stored. If an evacuated container is partially filled withA liquid, a portion of liquid evaporates to fillthe remaining volume of the container withVapour. Initially the liquid evaporates andPressure exerted by vapours on the walls of The container (vapour pressure) increases. AfterSome time it becomes constant, an equilibriumls established between liquid phase andVapour phase. Vapour pressure at this stagels known as equilibrium vapour pressure orSaturated vapour pressure.. Since process ofVapourisation is temperature dependent; the Temperature must be mentioned whilereporting the vapour pressure of a liquid.
When a liquid is heated in an open vessel,The liquid vapourises from the surface. At theTemperature at which vapour pressure of theLiquid becomes equal to the external pressure,Vapourisation can occur throughout the bulkOf the liquid and vapours expand freely intoThe surroundings. The condition of freeVapourisation throughout the liquid is calledBoiling. The temperature at which vapourPressure of liquid is equal to the externalPressure is called boiling temperature at thatPressure. At 1 atm pressure boilingTemperature is called normal boiling point.If pressure is 1 bar then the boiling point isCalled standard boiling point of the liquid. Standard boiling point of the liquid is slightlyLower than the normal boiling point because 1 bar pressure is slightly less than 1 atmPressure . The normal boiling point of water is $100^{\circ} C (373 K)$, its standard boiling point is $99.6^{\circ} C (372.6 K)$.At high altitudes atmospheric pressure isLow. Therefore liquids at high altitudes boil atLower temperatures in comparison to that atSea level. Since water boils at low temperatureOn hills, the pressure cooker is used forCooking food. In hospitals surgical instrumentsAre sterilized in autoclaves in which boilingPoint of water is increased by increasing thePressure above the atmospheric pressure byUsing a weight covering the vent.Boiling does not occur when liquid isHeated in a closed vessel. On heatingContinuously vapour pressure increases.
AtFirst a clear boundary is visible between liquidAnd vapour phase because liquid is more denseThan vapour. As the temperature increases more and more molecules go to vapour phaseAnd density of vapours rises. At the same timeLiquid becomes less dense. It expands becauseMolecules move apart. When density of liquidAnd vapours becomes the same; the clearBoundary between liquid and vapoursDisappears. This temperature is called critical Temperature.
  1. First complete data on Pressure-Volume-Temperature relations of a substance in both Gaseous and liquid state was obtained by:
  1. Thomas Andrews
  2. Fritz London
  3. Robert Boyle
  4. Joseph Lewis Gay Lussac
  1. Critical Temperature (TC) of carbon dioxide is.....
  1. $24^\circ C$
  2. $30.8^\circ C$
  3. $56^\circ C$
  4. $29^\circ C$
  1. The condition of free Vapourisation throughout the liquid is called …
  1. Evaporation
  2. Melting
  3. Boiling
  4. None of above
  1. Standard boiling point of Water is....
  1. $100^\circ C$
  2. $3^\circ C$
  3. $105^\circ C$
  4. $99.6^\circ C$
  1. Boundary between liquid and vapours Disappears,This temperature is called …
  1. Critical temperature
  2. Absolute temperature
  3. Normal temperature
  4. Boiling temperature
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Q 295 Marks Questions5 Marks
Pay load is defined as the difference between the mass of displaced air and the mass of the balloon. Calculate the pay load when a balloon of radius $10 \ m$ , mass $100 \ kg$ is filled with helium at 1.66 bar at $27^{\circ} C$. (Density of air $=1.2 kg$ $m ^{-3}$ and $R =0.083 bar dm ^3 K^{-1} mol^{-1}$ ).
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Q 305 Marks Questions5 Marks
Pressure of $1$ g of an ideal gas A at $27^{\circ} C$ is found to be $2$ bar. When $2$ g of another ideal gas B is introduced in the same flask at same temperature the pressure becomes $3$ bar. Find a relationship between their molecular masses.
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Q 335 Marks Questions5 Marks
What will be the pressure of the gaseous mixture when 0.5 L of $\mathrm{H}_2$ at 0.8 bar and 2.0 L of dioxygen at 0.7 bar are introduced in a 1 L vessel at $27^{\circ} \mathrm{C}$ ?
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