MCQ Questions For Class 11 Chemistry Chapter 5 States of Matter

Please refer to MCQ Questions States of Matter for Chapter 5 Class 11 Chemistry given below. All MCQ questions are provided with answers. These MCQ Questions for Class 11 Chemistry are designed based on the chapters given in your CBSE NCERT Textbook for Class 11 Chemistry. These MCQ Questions are expected to come in your class 11 Board exams.

Question. Which of the following statements is wrong for gases?                                                           
(a) Confined gas exerts uniform pressure on the walls of its container in all directions.
(b) Volume of the gas is equal to volume of container confining the gas.
(c) Gases do not have a definite shape and volume.
(d) Mass of a gas cannot be determined by weighing a container in which it is enclosed.

Question. At 25°C and 730 mm pressure, 380 mL of dry oxygen was collected. If the temperature is constant, what volume will the oxygen occupy at 760 mm pressure?                                               
(a) 569 mL
(b) 365 mL
(c) 265 mL
(d) 621 mL 

Question. Pressure remaining the same, the volume of a given mass of an ideal gas increases for every degree centrigrade rise in temperature by definite fraction of its volume at                                                 
(a) 0°C
(b) its critical temperature
(c) absolute zero
(d) its Boyle temperature.

Question. Dipole-induced dipole interactions are present in which of the following pairs?                                           
(a) HCl and He atoms
(b) SiF₄ and He atoms
(c) H₂O and alcohol
(d) Cl₂ and CCl₄

 Question. Which one of the following is the correct order ofinteractions?                                                               
(a) Covalent < hydrogen bonding < van der Waals’ < dipole-dipole
(b) van der Waals’ < hydrogen bonding < dipoledipole < covalent
(c) van der Waals’ < dipole-dipole < hydrogen bonding < covalent
(d) Dipole-dipole < van der Waals’ < hydrogen bonding < covalent.

Question. A mixture of N₂ and Ar gases in a cylinder contains 7 g of N₂ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of N₂ is [Use  tomic masses (in g mol–1) : N = 14, Ar = 40]                                                                 
(a) 9 bar
(b) 12 bar
(c) 15 bar
(d) 18 bar.

 Question. What is the density of N₂ gas at 227°C and 5.00 atm pressure? (R = 0.082 L atm K^–1mol^–1)                         
(a) 1.40 g/mL
(b) 2.81 g/mL
(c) 3.41 g/mL
(d) 0.29 g/mL

Question. 50 mL of each gas A and of gas B takes 150 and 200 seconds respectively for effusing through a pin holeunder the similar conditions. If molecular mass of  gas B is 36, the  olecular  ass of gas A will be                           
(a) 96
(b) 128
(c) 32
(d) 64 

Question. A certain gas takes three times as long to effuse out as helium. Its molecular mass will be 5 States of Matter                                                         
(a) 27 u
(b) 36 u
(c) 64 u
(d) 9 u 

Question. Two gases A and B having the same volume diffuse through a porous partition in 20 and 10 seconds respectively. The molecular mass of A is 49 u. Molecular mass of B will be                                                     
(a) 50.00 u
(b) 12.25 u
(c) 6.50 u
(d) 25.00 u 

Question. The volume occupied by 1.8 g of water vapour at 374°C and 1 bar pressure will be [Use R = 0.083 bar L K–1mol–1]                                                           
(a) 96.66 L
(b) 55.87 L
(c) 3.10 L
(d) 5.37 L

Question. Equal moles of hydrogen and oxygen gases are placed in a container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for ne- half of the hydrogen to escape?           
(a) 3/8
(b) 1/2
(c) 1/8
(d) 1/4

Question. A gaseous mixture was prepared by taking equal oles of CO and N₂. If the total pressure of the mixture was found 1 atmosphere, the partial pressure of the nitrogen (N₂) in the  ixture is                                                         
(a) 0.5 atm
(b) 0.8 atm
(c) 0.9 atm
(d) 1 atm 

Question. Which of the following mixtures of gases does not obey Dalton’s law of partial pressure?                           
(a) Cl₂ and SO₂
(b) CO₂ and He
(c) O₂ and CO₂
(d) N₂ and O₂ 

Question. At what temperature, the rate of effusion of N₂ would be 1.625 times than the rate of SO₂ at 50°C?           
(a) 373°C
(b) 620°C
(c) 100°C
(d) 173°C

Question. 50 mL of hydrogen diffuses out through a small hole of a vessel, in 20 minutes. The time taken by 40 mL of oxygen to diffuse out is                                                       
(a) 32 minutes
(b) 64 minutes
(c) 8 minutes
(d) 12 minutes

Question. Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of 1 atm but also a concentration of 1 mole litre–1? (R = 0.082 litre atm mol–1 deg–1)                                                 
(a) At STP
(b) When V = 22.4 litres
(c) When T = 12 K
(d) Impossible under any conditions

Question. A bubble of air is underwater at temperature 15°C and the pressure 1.5 bar. If the bubble rises to the surface where the temperature is 25°C and the pressure is 1.0 bar, what will  appen to the volume of the bubble?     
(a) Volume will become greater by a factor of 1.6.
(b) Volume will become greater by a factor of 1.1.
(c) Volume will become smaller by a factor of 0.70.
(d) Volume will become greater by a factor of 2.5.

Question. The pressure exerted by 6.0 g of methane gas in a 0.03 m3 vessel at 129°C is (Atomic masses: C = 12.01, H = 1.01 and R = 8.314 J K–1 mol–1)                                     
(a) 215216 Pa
(b) 13409 Pa
(c) 41648 Pa
(d) 31684 Pa 

Question. At constant temperature, in a given mass of an ideal gas                                                               
(a) the ratio of pressure and volume always remains constant
(b) volume always remains constant
(c) pressure always remains constant
(d) the product of pressure and volume always remains constant.

Question. If P, V, M, T and R are pressure, volume, molar mass, temperature and gas constant respectively, then for an ideal gas, the density is given by                                         
(a) RT PM
(b) P RT
(c) M V
(d) PM RT  

Question. By what factor does the average velocity of a gaseous molecule increase when the temperature (in Kelvin) is doubled?                                                     
(a) 2.0
(b) 2.8
(c) 4.0
(d) 1.4

Question. Root mean square velocity of a gas molecule is proportional to                                                   
(a) m^1/2
(b) m⁰
(c) m^–1/2
(d) m

Question. The correct value of the gas constant ‘R’ is close to                                                     
(a) 0.082 litre-atmosphere K
(b) 0.082 litre-atmosphere K^–1 mol^–1
(c) 0.082 litre-atmosphere^–1 K mol^–1
(d) 0.082 litre–1 atmosphere^–1 K mol. 

Question. Select one correct statement. In the gas equation, PV = nRT                                                           
(a) n is the number of molecules of a gas
(b) V denotes volume of one mole of the gas
(c) n moles of the gas have a volume V
(d) P is the pressure of the gas when only one mole of gas is present. 

Question. If a gas expands at constant temperature, it indicates that                                                       
(a) kinetic energy of molecules remains the same
(b) number of the molecules of gas increases
(c) kinetic energy of molecules decreases
(d) pressure of the gas increases. 

Question. At STP, 0.50 mol H₂ gas and 1.0 mol He gas                                               
(a) have equal average kinetic energies
(b) have equal molecular speeds
(c) occupy equal volumes
(d) have equal effusion rates.

Question. A closed flask contains water in all its three states solid, liquid and vapour at 0°C. In this situation, the average kinetic energy of water molecules will be                                                       
(a) the greatest in all the three states
(b) the greatest in vapour state
(c) the greatest in the liquid state
(d) the greatest in the solid state.

Question. A gas at 350 K and 15 bar has molar volume 20 percent smaller than that for an ideal gas under the same conditions. The correct option about the gas and its compressibility factor  Z) is                                                           
(a) Z < 1 and repulsive forces are dominant
(b) Z > 1 and attractive forces are dominant
(c) Z > 1 and repulsive forces are dominant
(d) Z < 1 and attractive forces are dominant.

Question. A gas such as carbon monoxide would be most likely to obey the ideal gas law at                                       
(a) low temperatures and high pressures
(b) high temperatures and high pressures
(c) low temperatures and low pressures
(d) high temperatures and low pressures. 

Question. Maximum deviation from ideal gas is expected from                                                     
(a) CH₄(g)
(b) NH₃(g)
(c) H₂(g)
(d) N₂(g)

Question. Average molar kinetic energy of CO and N₂ at same temperature is                                                       
(a) KE₁ = KE₂
(b) KE₁ > KE₂
(c) KE₁ < KE₂
(d) can’t say anything. Both volumes are not given. 

Question. The average kinetic energy of an ideal gas, per molecule in S.I. units, at 25°C will be                                     
(a) 6.17 × 10^–20 J
(b) 7.16 × 10^–20 J
(c) 61.7 × 10^–20 J
(d) 6.17 × 10^–21 J

Question. van der Waals’ real gas, acts as an ideal gas, at which conditions?                                           
(a) High temperature, low pressure
(b) Low temperature, high pressure
(c) High temperature, high pressure
(d) Low temperature, low pressure

Question. Given van der Waals’ constant for NH₃, H₂, O₂ and CO₂ are respectively 4.17, 0.244, 1.36 and 3.59, which one of the following gases is most easily liquefied?                                               
(a) NH₃
(b) H₂
(c) O₂
(d) CO₂ 

Question. An ideal gas, obeying kinetic theory of gases cannot be liquefied, because                                               
(a) it solidifies before becoming a liquid
(b) forces acting between its molecules are negligible
(c) its critical temperature is above 0°C
(d) its molecules are relatively small in size.

Question. The beans are cooked earlier in pressure cooker because                                                         
(a) boiling point increases with increasing pressure
(b) boiling point decreases with increasing pressure
(c) extra pressure of pressure cooker softens the beans
(d) internal energy is not lost while cooking in pressure cooker.

Question. When is deviation more in the behaviour of a gas from the ideal gas equation PV = nRT?                         
(a) At high temperature and low pressure
(b) At low temperature and high pressure
(c) At high temperature and high pressure
(d) At low temperature and low pressure 

Question. A gas is said to behave like an ideal gas when the relation PV/T = constant. When do you expect a real gas to behave like an ideal gas?                                           
(a) When the temperature is low.
(b) When both the temperature and pressure are low.
(c) When both the temperature and pressure are high.
(d) When the temperature is high and pressure is low.

Question. Which of the following is not a type of van der Waal’s forces?                                         
(a) Dipole – dipole forces
(b) Dipole – induced dipole forces
(c) Ion – dipole forces
(d) London forces

Question. Who proposed the concept of dispersion force ?                                         
(a) Heitler and London
(b) van der Waal
(c) Gay Lussac
(d) Fritz London

Question. The interaction energy of London force is inversely proportional to sixth power of the distance between two interacting particles but their magnitude depends upon                                             
(a) charge of interacting particles
(b) mass of interacting particles
(c) polarisability of interacting particles
(d) strength of permanent dipoles in the particles.

Question. London forces are always …I… and interaction energy is inversely proportional to the …II… power of the distance between two interacting particles. Here, I and II refer to                                           
(a) I → repulsive, II → sixth
(b) I →  attractive,II →  fourth
(c) I →  attractive,II →  sixth
(d) I →  repulsive, II →  fourth

Question. Dipole-dipole forces act between the molecules possessing permanent dipole. Ends of dipoles possess ‘partial charges’. The partial charge is                                         
(a) more than unit electronic charge
(b) equal to unit electronic charge
(c) less than unit electronic charge
(d) double the unit electronic charge

Question. Dipole-dipole interaction is stronger than the London forces but is weaker than ion-ion interaction because                                           
(a) only partial charges are involved
(b) only total charges are involved
(c) both (a) and (b)
(d) sometimes (a) and sometimes (b)

Question. Induced dipole moment depend upon the I. dipole moment present in the permanent dipole. II polarisability of the electrically neutral molecules. Identify the correct option.                                     
(a) I is correct but II is wrong
(b) I is wrong and II is correct
(c) Both I and II are wrong
(d) Both I and II are correct

Question. Dipole-induced dipole interactions are present in which of the following pairs :                                           
(a) Cl₂ and CCl₄
(b) HCl and He atoms
(c) SiF₄ and He atoms
(d) H₂O and alcohol

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

Question. Which of the following statements regarding thermal energy is correct?                                                 
(a) Thermal energy is the measure of average kinetic energy of the particles of the matter and is thus responsible for movement of particles.
(b) Intermolecular forces tend to keep the moleculestogether but thermal energy of the molecules tends to  keep them apart.
(c) Three states of matter are the result of balance between intermolecular forces and the thermal energy of the molecules.
(d) All of the above