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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
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
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
Answer
Answer: (b) 50
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
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
Answer
Answer: (a) 2 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
Answer
Answer: (c) 36
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
Answer
Answer: (c) 1.34 g L-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
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) \(\frac {x}{4}\)
Answer
Answer: (a) x
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
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
Answer
Answer: (b) decreases
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
Answer
Answer: (c) 1 : 4
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
Answer
Answer: (a) 25.215 atm
Question 14.
Which of the following exhibits the weakest molecular forces?
(a) NH3
(b) HCl
(c) He
(d) H2O
Answer
Answer: (c) He
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
Answer
Answer: (d) 280 ml
Question 16.
Triple point of water is
(a) 273 K
(b) 373 K
(c) 203 K
(d) 193 K
Answer
Answer: (a) 273 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
Answer
Answer: (b) 2 : 5
Question 18.
Steam distillation is based on
(a) Boyle’s Law
(b) Charle’s Law
(c) Dalton’s Law of partial pressures
(d) Avogadro’s Law
Answer
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
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
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
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
Answer
Answer: (b) 0.50 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
Answer
Answer: (a) 8 : 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).
Answer
Answer: (c)
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
Answer
Answer: (c) 4 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
Answer
Answer: (d) CO2
Question 27.
Gas equation PV = nRT is obeyed by
(a) Only isothermal process
(b) Only adiabatic process
(c) Both (a) and (b)
(d) None of these
Answer
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
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
Answer
Answer: (c) H2
Question 30.
When the temperature is increased, surface tension of water
(a) increases
(b) decreases
(c) remains constant
(d) shows irregular behaviour
Answer
Answer: (b) decreases
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
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
Answer
Answer: (c) CO2
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
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 ……………….
Answer
Answer: together, apart
Question 2.
The force of attraction between two temporary dipoles is known as ……………….
Answer
Answer: London or dispersion forces
Question 3.
Attractive forces operating between the polar molecules having permanent dipole and the molecules lacking permanent dipole are called ……………….
Answer
Answer: dipole-induced dipole forces
Question 4.
Dipole-dipole forces act between the molecules possessing ……………….
Answer
Answer: permanent dipole
Question 5.
Hydrogen bond is a special case of ………………. interactions.
Answer
Answer: dipole-dipole
Question 6.
At constant temperature, the pressure of a fixed amount of a gas varies ………………. with its volume.
Answer
Answer: inversely
Question 7.
Each line of the volume vs temperature graph at constant pressure is called ……………….
Answer
Answer: Isobar
Question 8.
The lowest hypothetical or imaginary temperature at which gases are supposed to occupy ………………. volume is called absolute zero.
Answer
Answer: zero
Question 9.
At constant volume, ………………. of a fixed amount of a gas varies directly with the ……………….
Answer
Answer: pressure, temperature
Question 10.
Equal volumes of all gases under similar conditions of temperature and pressure contain ………………. of molecules.
Answer
Answer: equal number
True/False Statements
Question 1.
The Charles law shows the variation of volume with pressure at constant temperature.
Answer
Answer: False
Question 2.
Equal volumes of all gases contain equal number of molecules under different conditions of temperature and pressure.
Answer
Answer: False
Question 3.
The gases deviate from ideal behaviour at low temperatures and high pressures.
Answer
Answer: True
Question 4.
The real gases obey van der Waals equation of state.
Answer
Answer: True
Question 5.
The viscosity of the liquids increases with increase in temperature.
Answer
Answer: False
Question 6.
The surface tension of liquids usually decreases with decrease in temperature.
Answer
Answer: False
Question 7.
Boyle’s law states that under isothermal conditions, pressure of a fixed amount of a gas is inversely proportional to its volume.
Answer
Answer: True
Question 8.
Liquids have definite volume because molecules do not separate from each other.
Answer
Answer: True
Question 9.
Normal boiling point and standard boiling point of a liquid is one and the same thing.
Answer
Answer: False
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.
Answer
Answer: False
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 |
Answer
Answer:
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. |
Answer
Answer:
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 |
Answer
Answer:
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 |
Answer
Answer:
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 |
Answer
Answer:
Column I | Column II |
1. 0°C, 1 bar pressure | (ii) 22700 mL |
2. 0°C, 1 atm pressure | (i) 22400 mL |
3. 25°C, 1 bar pressure | (iii) 24800 mL |
4. 25°C, 1 atm pressure | (iv) 24480 mL |
Column I | Column II |
1. CO | (i) 154 |
2. CO2 | (ii) 134 |
3. CH4 | (iii) 304 |
4. O2 | (iv) 191 |
Answer
Answer:
Column I | Column II |
1. CO | (ii) 134 |
2. CO2 | (iii) 304 |
3. CH4 | (iv) 191 |
4. O2 | (i) 154 |
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