Class 11 Chemistry · 55 questions · 50 with answers
A person living in Shimla observed that cooking food without using pressure cooker takes more time. The reason for this observation is that at high altitude:
(iii) pressure decreases
Which of the following property of water can be used to explain the spherical shape of rain droplets?
(ii) surface tension
A plot of volume (V ) versus temperature (T ) for a gas at constant pressure is a straight line passing through the origin. The plots at different values of pressure are shown in Fig. 5.1. Which of the following order of pressure is correct for this gas?
This question refers to a figure in the original PDF.
(iii) p1 < p2 < p3 < p4 Fig. 5.1
The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon
(iii) polarisability of interacting particles
Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess ‘partial charges’. The partial charge is
(iii) less than unit electronic charge
The pressure of a 1:4 mixture of dihydrogen and dioxygen enclosed in a vessel is one atmosphere. What would be the partial pressure of dioxygen?
(iii) 8×10 Nm
As the temperature increases, average kinetic energy of molecules increases. What would be the effect of increase of temperature on pressure provided the volume is constant?
(i) increases
Gases possess characteristic critical temperature which depends upon the magnitude of intermolecular forces between the particles. Following are the critical temperatures of some gases. Gases H2 He O2 N2 Critical temperature in Kelvin 33.2 5.3 154.3 126 From the above data what would be the order of liquefaction of these gases? Start writing the order from the gas liquefying first
(iv) O2, N2, H2, He
What is SI unit of viscosity coefficient (η)?
(ii) Nsm–2
Atmospheric pressures recorded in different cities are as follows: Cities Shimla Bangalore Delhi Mumbai p in N/m2 1.01×105 1.2×105 1.02×105 1.21×105 Consider the above data and mark the place at which liquid will boil first.
(i) Shimla
Which curve in Fig. 5.2 represents the curve of ideal gas?
This question refers to a figure in the original PDF.
(i) B only
Increase in kinetic energy can overcome intermolecular forces of attraction. How will the viscosity of liquid be affected by the increase in temperature?
This question refers to a figure in the original PDF.
(iii) Decrease
How does the surface tension of a liquid vary with increase in temperature?
(ii) Decreases
With regard to the gaseous state of matter which of the following statements are correct?
(ii) Complete disorder of molecules
(iii) Random motion of molecules
Which of the following figures does not represent 1 mole of dioxygen gas at STP?
(i) 16 grams of gas
(iv) 11.2 litres of gas
Under which of the following two conditions applied together, a gas deviates most from the ideal behaviour?
(ii) High pressure
(iii) Low temperature
Which of the following changes decrease the vapour pressure of water kept in a sealed vessel?
(ii) Adding salt to water
(iv) Decreasing the temperature of water
If 1 gram of each of the following gases are taken at STP, which of the gases will occupy
(a) greatest volume and
(b) smallest volume? CO, H2O, CH4, NO
Physical properties of ice, water and steam are very different. What is the chemical composition of water in all the three states.
Remains the same i.e., H2O.
The behaviour of matter in different states is governed by various physical laws. According to you what are the factors that determine the state of matter?
Pressure, temperature, mass and volume
Use the information and data given below to answer the questions
(a) to
(b) Looking at the trend of boiling points of HCl, HBr and HI, explain out of dipole-dipole interaction and London interaction, which one is predominant here. (c) Why is boiling point of hydrogen fluoride highest while that of hydrogen chloride lowest?
(c) : • Stronger intermolecular forces result in higher boiling point. • Strength of London forces increases with the number of electrons in the molecule. • Boiling point of HF, HCl, HBr and HI are 293 K, 189 K, 206 K and 238 K respectively. (a) Which type of intermolecular forces are present in the molecules HF, HCl, HBr and HI?
What will be the molar volume of nitrogen and argon at 273.15K and 1 atm?
22.4 litre
A gas that follows Boyle’s law, Charle’s law and Avogadro’s law is called an ideal gas. Under what conditions a real gas would behave ideally?
Low pressure and high temperature
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.
Gas ‘A’ is at or below its critical temperature and gas ‘B’ is at a temperature higher than critical temperature.
Value of universal gas constant (R) is same for all gases. What is its physical significance?
Unit of R depends upon those units in which p, V and T are measured, R= . If pressure is measured in Pascal, per mole volume is measured in m3 and temperature is measured in Kelven then. Units of ‘R’ are –1 –1 –1 –1 Pam3K mol or J mol K . Jule is the unit of work done so ‘R’ is work done per mole per kelvin. 65 States of Matter
One of the assumptions of kinetic theory of gases states that “there is no force of attraction between the molecules of a gas.” How far is this statement correct? Is it possible to liquefy an ideal gas? Explain.
In the absence of intermolecular forces of attraction, it will not be possible to liquefy ideal gas.
The magnitude of surface tension of liquid depends on the attractive forces between the molecules. Arrange the following in increasing order of surface tension : water, alcohol (C2H5OH) and hexane [CH3(CH2)4CH3)].
hexane < alcohol < water
Pressure exerted by saturated water vapour is called aqueous tension. What correction term will you apply to the total pressure to obtain pressure of dry gas?
PDry gas = PTotal – aqueous tension
Name the energy which arises due to motion of atoms or molecules in a body. How is this energy affected when the temperature is increased? 57 States of Matter
Thermal energy. It is a measure of average kinetic energy of particles. It increases with increase in temperature.
Name two intermolecular forces that exist between HF molecules in liquid state.
(i) Dipole - dipole interaction (ii) Hydrogen - bonding
One of the assumptions of kinetic theory of gases is that there is no force of attraction between the molecules of a gas. State and explain the evidence that shows that the assumption is not applicable for real gases.
Real gases can be liquefied on cooling and compressing proving that forces of attraction exist between the molecules.
Compressibility factor, Z, of a gas is given as Z =
(i) What is the value of Z for an ideal gas?
(ii) For real gas what will be the effect on value of Z above Boyle’s temperature?
The critical temperature (Tc) and critical pressure ( pc ) of CO2 are 30.98°C and 73 atm respectively. Can CO2 ( g) be liquefied at 32°C and 80 atm pressure?
CO2 cannot be liquefied at 32°C by applying a pressure of 80 atm. This is because the temperature is greater than critical temperature of CO2.
For real gases the relation between p, V and T is given by van der Waals equation: ⎛ an 2 ⎞ ⎜⎝ p + 2 ⎟⎠ (V -nb) = nRT where ‘a’ and ‘b’ are van der Waals constants, ‘nb’ is approximately equal to the total volume of the molecules of a gas. ‘a’ is the measure of magnitude of intermolecular attraction.
(i) Arrange the following gases in the increasing order of ‘b’. Give reason. O2, CO2, H2, He
(ii) Arrange the following gases in the decreasing order of magnitude of ‘a’. Give reason. CH4, O2, H2
The relation between pressure exerted by an ideal gas (pideal) and observed pressure (preal) is given by the equation pideal = p real + 2 If pressure is taken in Nm–2, number of moles in mol and volume in m3, Calculate the unit of ‘a’. What will be the unit of ‘a’ when pressure is in atmosphere and volume in dm3?
pideal = p real + 2 We write the known units in the above equation. –2 –2 a . mol Nm = Nm + 3 2 (m ) If two values with same units are added then the units of result are same as added units. -2 a .mol ∴ Nm = 6 –2 6 Nm .m a = 2 a = Nm4 mol–2 Similarly, when p is in atm and volume in dm3 3 2 atm(dm ) a = 2 = atm dm6 mol–2
Name two phenomena that can be explained on the basis of surface tension.
(i) Rise or fall of the liquid in a capillary - capillary action. (ii) Spherical shape of small liquid drops.
Viscosity of a liquid arises due to strong intermolecular forces existing between the molecules. Stronger the intermolecular forces, greater is the viscosity. Name the intermolecular forces existing in the following liquids and arrange them in the increasing order of their viscosities. Also give reason for the assigned order in one line. Water, hexane (CH3CH2CH2CH2CH2CH3), glycerine (CH2OH CH(OH) CH2OH)
In water and glycerine – Hydrogen bonding. Hexane – Dispersion forces/ London forces. The order of viscosities of these liquids is hexane < water < glycerine. Hexane has weakest intermolecular forces and glycerine the strongest. (three OH groups). Therefore, hexane has minimum viscosity and glycerine has maximum viscosity.
Explain the effect of increasing the temperature of a liquid, on intermolecular forces operating between its particles, what will happen to the viscosity of a liquid if its temperature is increased?
The viscosity of a liquid decreases with the increase in temperature since the kinetic energy of the molecules can overcome intermolecular forces. So the liquid can flow more easily.
The variation of pressure with volume of the gas at different temperatures can be graphically represented as shown in Fig. 5.3. On the basis of this graph answer the following questions.
This question refers to a figure in the original PDF.
(i) How will the volume of a gas change if its pressure is increased at constant temperature?
Pressure versus volume graph for a real gas and an ideal gas are shown in Fig. 5.4. Answer the following questions on the basis of this graph.
This question refers to a figure in the original PDF.
Match the graphs between the following variables with their names : Graphs Names (i) Pressure vs temperature
(a) Isotherms graph at constant molar volume. (ii) Pressure vs volume graph
(c) Isochores at constant pressure.
(b) Constant temperature curve at constant temperature. (iii) Volume vs temperature graph
(d) Isobars
Match the following gas laws with the equation representing them. (i) Boyle’s law
(a) V ∝ n at constant T and p (ii) Charle’s law
(b) pTotal = p1 + p2 + p3+...... at constant T, V (iii) Dalton’s law
(d) V ∝ T at constant n and p (e) p∝ at constant n and T
(c) = Constant (iv) Avogadro law
Match the following graphs of ideal gas with their co-ordinates : Graphical representation x and y co-ordinates (i)
(a) pV vs. V (ii)
(b) p vs. V (iii)
(c) p vs.
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. (i) Both A and R are true and R is the correct explanation of A. (ii) Both A and R are true but R is not the correct explanation of A. (iii) A is true but R is false. (iv) A is false but R is true.
(i) Both A and R are true and R is the correct explanation of A.
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. (i) Both A and R are true and R is the correct explanation of A. (ii) Both A and R are true but R is not the correct explanation of A. (iii) A is true but R is false. (iv) A is false but R is true.
(ii) Both A and R are true but R is not the correct explanation of A.
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. (i) Both A and R are true and R is the correct explanation of A. (ii) Both A and R are true but R is not the correct explanation of A. (iii) A is true but R is false. (iv) A is false but R is true.
(iii) A is true but R is false.
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. (i) Both A and R are true and R is the correct explanation of A. (ii) Both A and R are true but R is not the correct explanation of A. (iii) A is true but R is false. (iv) A is false but R is true.
(i) Both A and R are true and R is the correct explanation of A.
Assertion (A): At critical temperature liquid passes into gaseous state imperceptibly and continuously. 61 States of Matter
Reason (R): The density of liquid and gaseous phase is equal to critical temperature. (i) Both A and R are true and R is the correct explanation of A. (ii) Both A and R are true but R is not the correct explanation of A. (iii) A is true but R is false. (iv) A is false but R is true.
(i) Both A and R are true and R is the correct explanation of A.
Assertion (A): Liquids tend to have maximum number of molecules at their surface.
Reason (R): Small liquid drops have spherical shape. (i) Both A and R are true and R is the correct explanation of A. (ii) Both A and R are true but R is not the correct explanation of A. (iii) A is true but R is false. (iv) A is false but R is true.
(iv) A is false but R is true.
Isotherms of carbon dioxide at various temperatures are represented in Fig. 5.5. Answer the following questions based on this figure.
This question refers to a figure in the original PDF.
(i) In which state will CO2 exist between the points a and b at temperature T1?
(ii) At what point will CO2 start liquefying when temperature is T1?
(iii) At what point will CO2 be completely liquefied when temperature is T2.
(iv) Will condensation take place when the temperature is T3. (v) What portion of the isotherm at T1 represent liquid and gaseous CO2 at equilibrium? Fig. 5.5
The variation of vapour pressure of different liquids with temperature is shown in Fig. 5.6.
This question refers to a figure in the original PDF.
(i) Calculate graphically boiling points of liquids A and B.
(ii) If we take liquid C in a closed vessel and heat it continuously. At what temperature will it boil?
(iii) At high altitude, atmospheric pressure is low (say 60 mm Hg). At what temperature liquid D boils?
(iv) Pressure cooker is used for cooking food at hill station. Explain in terms of vapour pressure why is it so? Fig. 5.6
Why does the boundary between liquid phase and gaseous phase disappear on heating a liquid upto critical temperature in a closed vessel? In this situation what will be the state of the substance?
Why does sharp glass edge become smooth on heating it upto its melting point in a flame? Explain which property of liquids is responsible for this phenomenon. 63 States of Matter
Explain the term ‘laminar flow’. Is the velocity of molecules same in all the layers in laminar flow? Explain your answer.
Isotherms of carbon dioxide gas are shown in Fig. 5.7. Mark a path for changing gas into liquid such that only one phase (i.e., either a gas or a liquid) exists at any time during the change. Explain how the temperature, volume and pressure should be changed to carry out the change. Fig. 5.7
This question refers to a figure in the original PDF.