# MCQ Questions for Class 11 Chemistry Chapter 5 States of Matter with Answers

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## States of Matter Class 11 MCQs Questions with Answers

Multiple Choice Type Questions

Question 1.
The density of neon will be highest at
(a) STP
(b) 0°C and 2 atm
(c) 273°C, 1 atm
(d) 273°C, 0.5 atm

Answer: (b) 0°C and 2 atm Question 2.
Rate of effusion of a gas is
(a) Directly proportional to its density
(b) Directly proportional to its molar mass
(c) Directly proportional to the square root of its mass
(d) Inversely proportional to the square root of its molar mass.

Answer: (d) Inversely proportional to the square root of its molar mass. Question 3.
A gas diffuses $$\frac {1}{5}$$ times as fast as hydrogen. Its molar mass is
(a) 25
(b) 50
(c) 25√2
(d) 50√2

Question 4.
The density of a gas is 4 times that of Y. If the molar mass M, that of Y is
(a) 2M
(b) $$\frac {M}{2}$$
(c) 4M
(d) $$\frac {M}{4}$$

Answer: (d) $$\frac {M}{4}$$

Question 5.
The pressure of 2 moles of an ideal gas at 273°C occupying a volume of 44.8 L is
(a) 2 atm
(b) 1 atm
(c) 3 atm
(d) 4 atm

Question 6.
What is the molar mass of C gas whose density is 1.5 g L-1 at 27°C and 1 atm pressure [R = 0.08 L atm K-1 mol-1].
(a) 360
(b) 720
(c) 36
(d) 18

Question 7.
At STP the density of nitrogen monoxide is
(a) 3.0 g L-1
(b) 30 gL-1
(c) 1.34 g L-1
(d) 2.68 gL-1

Question 8.
0.5 mole of each of H2, SO2 and CH4 are kept in a container. A hole was made in the container After 3 hours, the order of partial pressures in the container will be
(a) PsO2 > PCH4 > PH2
(b) PH2 > PSO2 > PCH4
(c) PCH4 > Pso2 > PH2
(d) PH2 > PcH4 > Pso2

Answer: (a) PsO2 > PCH4 > PH2

Question 9.
If r.sm.s. speed of gaseous molecules is x cm sec-1 at a pressure of p atm, then r.m.s. speed at a pressure of 2p atm and constant pressure will be
(a) x
(b) 2x
(c) 4x
(d) $$\frac {x}{4}$$

Question 10.
For an ideal gas, number of moles per litre in terms of its pressure P, gas constant R and temperature T is
(a) $$\frac {PT}{R}$$
(b) PRT
(c) $$\frac {P}{RT}$$
(d) $$\frac {RT}{P}$$

Answer: (c) $$\frac {P}{RT}$$

Question 11.
When temperature is increased, surface tension of water
(a) increases
(b) decreases
(c) remains constant
(d) shows irregular behaviour

Question 12.
Density ratio of O2 and H2 is 16 : 1. The ratio of their r.m.s velocities will be
(a) 4 : 1
(b) 1 : 16
(c) 1 : 4
(d) 16 : 1

Question 13.
Pressure of mixture of 4 g of O2 and 2 g of H2 confined in a bulb of 1 litre at 0 C is
(a) 25.215 atm
(b) 31.2015 atm
(c) 45.215 atm
(d) 15.210 atm

Question 14.
Which of the following exhibits the weakest molecular forces?
(a) NH3
(b) HCl
(c) He
(d) H2O

Question 15.
If 300 ml of a gas at 27C is cooled to 7°C at constant pressure, its final volume will be
(a) 135 ml
(b) 1540 ml
(c) 350 ml
(d) 280 ml

Question 16.
Triple point of water is
(a) 273 K
(b) 373 K
(c) 203 K
(d) 193 K

Question 17.
If the ratio of the masses of SO3 and O2 gases confined in a vessel is 1 : 1, then the ratio of their partial pressures would be
(a) 5 : 2
(b) 2 : 5
(c) 2 : 1
(d) 1 : 2
(e) 1 : 1

Question 18.
Steam distillation is based on
(a) Boyle’s Law
(b) Charle’s Law
(c) Dalton’s Law of partial pressures

Answer: (c) Dalton’s Law of partial pressures

Question 19.
Equal masses of methane and oxygen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by oxygen is
(a) $$\frac {1}{2}$$
(b) $$\frac {2}{3}$$
(c) $$\frac {1}{2}$$ × $$\frac {273}{298}$$
(d) $$\frac {1}{3}$$

Answer: (d) $$\frac {1}{3}$$

Question 20.
Equation for Boyle’s law is
(a) $$\frac {dP}{P}$$ = $$\frac {-dV}{V}$$
(b) $$\frac {dP}{P}$$ × $$\frac {dV}{V}$$
(c) $$\frac {d^2P}{P}$$ × $$\frac {dV}{dT}$$
(d) $$\frac {d^2P}{P}$$ × $$\frac {d^2V}{dT}$$

Answer: (a) $$\frac {dP}{P}$$ = $$\frac {-dV}{V}$$

Question 21.
Molar volume of CO2 is maximum at
(a) N.T.P.
(b) d°C and 2.0 atm
(c) 127°C and 1 atm
(d) 273°C and 2 atm

Answer: (d) 273°C and 2 atm

Question 22.
If a mixture of CO and N2 in equal amount have total 1 atm pressure, then partial pressure of N2 in the mixture is
(a) 1 atm
(b) 0.50 atm
(c) 2 atm
(d) 3 atm

Question 23.
A 4 : 1 mixture of helium and methane is contained in a vessel at 10 bar pressure. Due to a hole in the vessel, the gas mixture leaks out. The composition of the mixture effusing out initially is
(a) 8 : 1
(b) 8 : 3
(c) 4 : 1
(d) 1 : 1
(e) 2 : 1

Question 24.
Which of the following diagram correctly describes the behaviour of a fixed mass of an ideal gas? (T is measured in K). Question 25.
The temperature and pressure of 4 dm³ of CO2 gas are doubled. Then the volume of CO2 gas would be
(a) 2 dm³
(b) 3 dm³
(c) 4 dm³
(d) 8 dm³

Question 26.
4.4 g of a gas at STP occupies a volume of 2.24 L, the gas can be
(a) O2
(b) CO
(c) NO2
(d) CO2

Question 27.
Gas equation PV = nRT is obeyed by
(a) Only isothermal process
(c) Both (a) and (b)
(d) None of these

Answer: (c) Both (a) and (b)

Question 28.
The compressibility of a gas is less than unity at STP. Therefore
(a) Vm > 22.4 litres
(b) Vm < 22.4 litres
(c) Vm = 22.4 litres
(d) Vm = 44.8 litres

Answer: (c) Vm = 22.4 litres

Question 29.
If the four tubes of a car are filled to the same pressure with N2, O2, H2 and Ne separately, then which one will be filled first?
(a) N2
(b) O2
(c) H2
(d) Ne

Question 30.
When the temperature is increased, surface tension of water
(a) increases
(b) decreases
(c) remains constant
(d) shows irregular behaviour

Question 31.
The van der Waals equation reduces itself to the ideal gas equation at
(a) high pressure and low temperature
(b) low pressure and low temperature
(c) low pressure and high temperature
(d) low pressure and low temperature

Answer: (c) low pressure and high temperature

Question 32.
The density of a gas is 1.964 g dm-3 at 273 K and 76 cm Hg. The gas is
(a) CH4
(b) C2H6
(c) CO2
(d) Xe

Question 33.
Dominance of strong repulsive forces among the molecules of the gas (Z = compressibility factor)
(a) depends on Z and indicated by Z = 1
(b) depends upon Z and indicated by Z > 1
(c) depends on Z and indicated by Z < 1
(d) is independent of Z

Answer: (b) depends upon Z and indicated by Z > 1

Fill in the Blanks

Question 1.
Intermolecular forces tend to keep the molecules ………………. but thermal’energy of the molecules tends to keep them ……………….

Question 2.
The force of attraction between two temporary dipoles is known as ……………….

Question 3.
Attractive forces operating between the polar molecules having permanent dipole and the molecules lacking permanent dipole are called ……………….

Question 4.
Dipole-dipole forces act between the molecules possessing ……………….

Question 5.
Hydrogen bond is a special case of ………………. interactions.

Question 6.
At constant temperature, the pressure of a fixed amount of a gas varies ………………. with its volume.

Question 7.
Each line of the volume vs temperature graph at constant pressure is called ……………….

Question 8.
The lowest hypothetical or imaginary temperature at which gases are supposed to occupy ………………. volume is called absolute zero.

Question 9.
At constant volume, ………………. of a fixed amount of a gas varies directly with the ……………….

Question 10.
Equal volumes of all gases under similar conditions of temperature and pressure contain ………………. of molecules.

True/False Statements

Question 1.
The Charles law shows the variation of volume with pressure at constant temperature.

Question 2.
Equal volumes of all gases contain equal number of molecules under different conditions of temperature and pressure.

Question 3.
The gases deviate from ideal behaviour at low temperatures and high pressures.

Question 4.
The real gases obey van der Waals equation of state.

Question 5.
The viscosity of the liquids increases with increase in temperature.

Question 6.
The surface tension of liquids usually decreases with decrease in temperature.

Question 7.
Boyle’s law states that under isothermal conditions, pressure of a fixed amount of a gas is inversely proportional to its volume.

Question 8.
Liquids have definite volume because molecules do not separate from each other.

Question 9.
Normal boiling point and standard boiling point of a liquid is one and the same thing.

Question 10.
The total pressure exerted by the mixture of gases which react is equal to the sum of the partial pressures of individual gases.

Match Type Questions

 Column I Column II 1. Boyle’s Law (i) PV = kT 2. Charles’ Law (ii) V ∝ n 3. Avogadro Law (iii) PV = constant 4. Gay Lussac’s Law (iv) $$\frac {V}{T}$$ = constant

 Column I Column II 1. Boyle’s Law (iii) PV = constant 2. Charles’ Law (iv) $$\frac {V}{T}$$ = constant 3. Avogadro Law (ii) V ∝ n 4. Gay Lussac’s Law (i) PV = kT

 Column I Column II 1. London forces (i) Special case of dipole-dipole interactions 2. Dipole-dipole forces (ii) Molecules having and lacking permanent dipole. 3. Dipole-induced dipole-forces (iii) Molecules with permanent dipole. 4. Hydrogen bond (iv) Force of attraction between two temporary dipoles.

 Column I Column II 1. London forces (iv) Force of attraction between two temporary dipoles. 2. Dipole-dipole forces (iii) Molecules with permanent dipole. 3. Dipole-induced dipole-forces (ii) Molecules having and lacking permanent dipole. 4. Hydrogen bond (i) Special case of dipole-dipole interactions

 Column I Column II 1. Compressibility factor (i) Temperature at which a real gas obeys ideal gas law on largerange of pressure. 2. Boyle point (ii) Z = $$\frac {PV}{nRT}$$ 3. Ideal gas (iii) van der Waals equation 4. Real gas (iv) PV = nRT

 Column I Column II 1. Compressibility factor (ii) Z = $$\frac {PV}{nRT}$$ 2. Boyle point (i) Temperature at which a real gas obeys ideal gas law on largerange of pressure. 3. Ideal gas (iv) PV = nRT 4. Real gas (iii) van der Waals equation

 Column I Column II 1. Between phosphine molecules (i) London forces 2. Between neopentane molecules (ii) Dipole-induced dipole interactions 3. Between CH3 and HCl molecules (iii) Dipole-dipole interactions 4. Between NH3 molecules (iv) Hydrogen bonding

 Column I Column II 1. Between phosphine molecules (iii) Dipole-dipole interactions 2. Between neopentane molecules (i) London forces 3. Between CH3 and HCl molecules (ii) Dipole-induced dipole interactions 4. Between NH3 molecules (iv) Hydrogen bonding

 Column I Column II 1. 0°C, 1 bar pressure (i) 22400 mL 2. 0°C, 1 atm pressure (ii) 22700 mL 3. 25°C, 1 bar pressure (iii) 24800 mL 4. 25°C, 1 atm pressure (iv) 24480 mL