States of Matter Class 11 MCQ is one of the best strategies to prepare for the CBSE Class 11 Board exam. If you want to complete a grasp concept or work on one’s score, there is no method except constant practice. Students can improve their speed and accuracy by doing more MCQs on States of Matter Class 11, which will help them all through their board tests.
States of Matter Class 11 MCQ Question with Answers
Class 11 Chemistry MCQ with answers are given here to Chapter 5 States of Matter. These MCQs are based on the latest CBSE board syllabus and relate to the latest Class 11 Chemistry syllabus. By Solving these Class 11 MCQs, you will be able to analyze all of the concepts quickly in the chapter and get ready for the Class 11 Annual exam.
Learn Class 11 States of Matter MCQs with answers pdf free download according to the latest CBSE and NCERT syllabus. Students should prepare for the examination by solving CBSE Class 11 Chemistry States of Matter MCQ with answers given below
Question 1. 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 2. 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 3. 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
(b) its critical temperature
(c) absolute zero
(d) its Boyle temperature.
Question 4. 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
Question 5. 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 6. 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 7. 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 8. 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 9. 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 10. 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 11. 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 12. 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 13. 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 14. 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 15. 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?
Question 16. 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 17. 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 18. At what temperature, the rate of effusion of N2 would be 1.625 times than the rate of SO2 at 50°C?
Question 19. 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 20. 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 21. By what factor does the average velocity of a gaseous molecule increase when the temperature (in Kelvin) is doubled?
Question 22. 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 23. Root mean square velocity of a gas molecule is proportional to
Question 24. 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 25. 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.
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Question 26. 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 27. 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 28. 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 29. 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 30. 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 31. Maximum deviation from ideal gas is expected from
Question 32. 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 33. 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 34. 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 35. 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 36. 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 37. Who proposed the concept of dispersion force ?
(a) Heitler and London
(b) van der Waal
(c) Gay Lussac
(d) Fritz London
Question 38. 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 39. 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?
Question 40. 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 41. 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 42. 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 43. 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 44. 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 45. 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 46. 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 47. Which of the following exhibits the weakest intermolecular forces ?
Question 48. 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
Question 49. 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
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Frequently Asked Question (FAQs)
How many MCQ questions are there in Class 11 chapter 5 Chemistry?
In Class 11 chapter 5 Chemistry, we have provided 49 Important MCQ Questions, But in the future, we will add more MCQs so that you can get good marks in the Class 11 exam.
Can we score good marks in Class 11 Chemistry with the help of States of Matter MCQ Questions?
Yes, MCQ Question is one of the best strategies to make your preparation better for the CBSE Board Exam. It also helps to know the student’s basic understanding of each chapter. So, You can score good marks in the Class 11 Chemistry exam.