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💥MDCAT/ECAT Chemistry Chapter-wise High-Yield Chemistry MCQs on Gaseous State 🧬| Exam-Focused, 🎯 💯 Exam Booster🚀 Practice & Win 190+! 📚 Topper’s Choice
1️⃣ According to Graham’s Law of diffusion, the ratio of diffusion of H₂ and O₂ are respectively:
🟥 a) 1:2
🟦 b) 2:1
🟩 c) 1:4
🟨 d) 4:1
2️⃣ Collection of gas over water is an example of:
🟥 a) Graham’s law
🟦 b) Dalton’s law
🟩 c) Avogadro’s law
🟨 d) Gay-Lussac law
3️⃣ The molar volume of oxygen gas is maximum at:
🟥 a) 0°C and 1 atm
🟦 b) 0°C and 2 atm
🟩 c) 25°C and 1 atm
🟨 d) 25°C and 2 atm
4️⃣ The volume of gas would be theoretically zero at:
🟥 a) 0°C
🟦 b) 0 K
🟩 c) 273 K
🟨 d) 273°C
5️⃣If Kelvin temperature of ideal gas is doubled and pressure reduced to half, the volume will:
🟥 a) Remains same
🟦 b) Double
🟩 c) Reduced to half
🟨 d) Four times ✅
6️⃣ The molar volume of oxygen gas is 22.4 dm³ at:
🟥 a) 0°C and 1 atm
🟦 b) 25°C and 0.5 atm
🟩 c) 0 K and 1 atm
🟨 d) 25 K and 0.5 atm
7️⃣ Under similar conditions CH₄ gas diffuses … faster than SO₂ gas:
🟥 a) 1.5 times
🟦 b) 2 times
🟩 c) 4 times
🟨 d) 16 times
8️⃣ Which statement is INCORRECT about gas molecules?
🟥 a) They have large spaces
🟦 b) They possess kinetic energy
🟩 c) Their collision is elastic
🟨 d) Their molar mass depends upon temperature
9️⃣ The diffusion rate of C₃H₈ and CO₂ are same because:
🟥 a) Both are polyatomic gases
🟦 b) Both are denser than air
🟩 c) Both have same molar mass
🟨 d) Both contain carbon atoms
1️⃣ 0️⃣ Real gas reaches ideal behavior at:
🟥 a) Low temperature and low pressure
🟦 b) High temperature and high pressure
🟩 c) Low temperature and high pressure
🟨 d) High temperature and low pressure
1️⃣ 1️⃣ If the ratio of the rates of diffusion of the two gases A and B is 4:1, the ratio of their densities is:
🟥 a) 1:16
🟦 b) 1:4
🟩 c) 1:8
🟨 d) 1:2
12. Relative rates of diffusion of two gases X and Y are 3:2. If the density of Y is 27, the density of X is:
🟥 a) 27
🟦 b) 54
🟩 c) 4
🟨 d) 12
13. 1 liter of a gas weighs 2 g at 300 K and 1 atm. If pressure is made 75 atm, at which temperature will 1 L weigh 1 g?
🟥 a) 450 K
🟦 b) 800 K
🟩 c) 600 K
🟨 d) 900 K
14. Above Boyle temperature real gases show __________ deviation from ideal gases:
🟥 a) Positive
🟦 b) Negative
🟩 c) No
🟨 d) Both positive and negative
15. What are the units of “b” in van der Waals equation?
🟥 a) L/mol
🟦 b) L mol
🟩 c) 1/L mol
🟨 d) L
16. The temperature at which a real gas obeys Boyle’s law or behaves ideally is called:
🟥 a) Boyle temperature
🟦 b) Charge temperature
🟩 c) Critical temperature
🟨 d) Absolute temperature
17. A gas of 2 moles occupies 500 ml at 300 K and 50 atm. Compressibility factor is:
🟥 a) 1.863
🟦 b) 0.7357
🟩 c) 0.5081
🟨 d) 1.8754
18. The term that corrects for attractive forces in van der Waals equation is:
🟥 a) nb
🟦 b) an²/V²
🟩 c) –an²/V²
🟨 d) –nb
19. The term “a/V²” in van der Waals equation is for:
🟥 a) Internal pressure
🟦 b) Intermolecular attraction
🟩 c) Temperature correction
🟨 d) Both a and b
20. In van der Waals equation of state, the term that accounts for intermolecular force is:
🟥 a) (V – b)
🟦 b) RT
🟩 c) (P + a/V²)
🟨 d) (RT)⁻¹
21. An ideal gas expands according to PV = constant. On expansion the temperature of gas:
🟥 a) Will rise
🟦 b) Will remain constant
🟩 c) Cannot be determined
🟨 d) Will drop
22. A gas at 100 K is heated until 200 K. What happens to kinetic energy?
🟥 a) Halved
🟦 b) Tripled
🟩 c) Quadrupled
🟨 d) Doubled
23. PV/nRT is known as:
🟥 a) Temperature factor
🟦 b) Compressibility factor
🟩 c) Pressure factor
🟨 d) Volume factor
24. The value of ‘b’ for CO₂ is 42.69 × 10⁻⁶ m³/mol. Volume of a molecule is:
🟥 a) 7.59 m³
🟦 b) 7.03 m³
🟩 c) 76.09 m³
🟨 d) 7.09 m³
25. Corresponding pressure of 32.8 psi in kPa is:
🟥 a) 226.085 kPa
🟦 b) 2.23 kPa
🟩 c) 1695.8 kPa
🟨 d) None of these
26. Low atmospheric system is called:
🟥 a) Depression
🟦 b) Atmosphere
🟩 c) Both of them
🟨 d) None of them
27. Which reduces force of attraction between gas molecules?
🟥 a) High pressure
🟦 b) High temperature
🟩 c) Low temperature
🟨 d) All of them
28. At STP, 44.8 L of any gas weighs equal to:
🟥 a) 1 mole
🟦 b) 1.5 mole
🟩 c) 2 mole
🟨 d) 3 mole
29. The random motion of gas molecules from one place to another is called:
🟥 a) Effusion
🟦 b) Osmosis
🟩 c) Diffusion
🟨 d) All of them
30. The escape of gas molecules through a tiny hole into an evacuated chamber is called:
🟥 a) Effusion
🟦 b) Osmosis
🟩 c) Diffusion
🟨 d) All of them
31. The collision of ideal gas molecules are:
🟥 a) Elastic
🟦 b) Inelastic
🟩 c) Both a and b
🟨 d) None of them
32. When the pressure approaches zero, all gases reach a value of Z ………..
🟥 a) Less than 1
🟦 b) Greater than 1
🟩 c) Equal to 1
🟨 d) None of them
33. Which increases force of attraction between gas molecules?
🟥 a) Low pressure
🟦 b) High temperature
🟩 c) Low temperature
🟨 d) All of them
34. Out of the following, which molecule does NOT possess London forces?
🟥 a) He
🟦 b) Ne
c) H₂
🟨 d) NH₃
35. The three variables of volume, pressure & temperature can be inter-related in one expression called:
🟥 a) Boyle’s law
🟦 b) Charles’s law
🟩 c) General gas law
🟨 d) Dalton’s law
36. The total pressure exerted by a mixture of gases is the sum of partial pressures of all gases. This is the statement of:
🟥 a) Dalton’s law
🟦 b) Gay-Lussac’s law
🟩 c) Avogadro’s law
🟨 d) Graham’s law
37. The respiration process in living things is an application of:
🟥 a) Gay-Lussac’s law
🟦 b) Graham’s law
🟩 c) Avogadro’s law
🟨 d) Dalton’s law
38. The partial pressure of oxygen in air is:
🟥 a) 159.6 mm Hg
🟦 b) 259.6 mm Hg
🟩 c) 359.6 mm Hg
🟨 d) None of them
39. The partial pressure of water vapours in gases is called:
🟥 a) Surface tension
🟦 b) Aqueous tension
🟩 c) Atmospheric pressure
🟨 d) None of them
40. The volume of reactant and product gases in a chemical reaction at given T and P are in small whole numbers. This is the statement of:
🟥 a) Gay-Lussac’s law
🟦 b) Graham’s law
🟩 c) Avogadro’s law
🟨 d) Ideal gas law
41. The density of a gas varies directly with:
🟥 a) Temperature
🟦 b) Volume
🟩 c) Pressure
🟨 d) All of them
42. The density of a gas varies inversely with:
🟥 a) Temperature
🟦 b) Molecular weight
🟩 c) Pressure
🟨 d) All of them
43. At same T and P, two balloons filled with CH₄ and SO₂. If SO₂ escapes at 100 ml/s, CH₄ escapes at:
🟥 a) 50 ml/s
🟦 b) 100 ml/s
🟩 c) 200 ml/s
🟨 d) 400 ml/s
44. At high altitude, pilots may have uncomfortable breathing in non-pressurized cabin where O₂ partial pressure is around:
🟥 a) 159.6 mm Hg
🟦 b) 150 mm Hg
🟩 c) 250 mm Hg
🟨 d) 100 mm Hg
45. Which property is same for both normal hydrogen and deuterium?
🟥 a) Boiling point
🟦 b) Freezing point
🟩 c) Bond energy
🟨 d) Bond length
46. For which type of gases the graph between P (x-axis) and PV/nRT (y-axis) is a horizontal line?
🟥 a) Ideal gases
🟦 b) Real gases
🟩 c) Noble gases
🟨 d) None of them
47. The molecular weight of a gas varies directly with:
🟥 a) Temperature
🟦 b) Volume
🟩 c) Pressure
🟨 d) None of them
48. Equation used to determine molecular weight of a gas if density is given:
🟥 a) M.W = RTd/P
🟦 b) M.W = P/RTd
🟩 c) M.W = RPd/T
🟨 d) None of them
49. The molecular weight of a gas varies inversely with:
🟥 a) Temperature
🟦 b) Molecular weight
🟩 c) Pressure
🟨 d) None of them
50. Which one of the following is a monoatomic gas?
🟥 a) Krypton
🟦 b) Hydrogen
🟩 c) Nitrogen
🟨 d) Fluorine
51. Which is an ideal gas?
🟥 a) CH₄
🟦 b) CO
🟩 c) CO₂
🟨 d) None of them
52. Which is a real gas?
🟥 a) H₂
🟦 b) O₂
🟩 c) He
🟨 d) All of them
53. A gas which does not obey gas laws at all T and P is called:
🟥 a) Perfect gas
🟦 b) Real gas
🟩 c) Noble gas
🟨 d) None of them
54. … temperature and … pressure make gases non-ideal:
🟥 a) Low, high
🟦 b) High, low
🟩 c) Low, low
🟨 d) High, high
55. Which one of the following is more ideal?
🟥 a) Polar gases
🟦 b) Non-polar gases
🟩 c) Real gases
🟨 d) None of them
56. Which one of the following is more non-ideal?
🟥 a) Polar gases
🟦 b) Non-polar gases
🟩 c) Inert gases
🟨 d) None of them
57. Attractive forces between gas molecules over short distances are called:
🟥 a) Induced dipole
🟦 b) van der Waals forces
🟩 c) Dipole-dipole force
🟨 d) All of them
58. van der Waals forces are:
🟥 a) Permanent forces
🟦 b) Temporary forces
🟩 c) Variable forces
🟨 d) None of them
59. Weak short-range attractive forces in non-polar molecules/inert gases due to temporary dipoles are:
🟥 a) London forces
🟦 b) Hydrogen bonding
🟩 c) Induced forces
🟨 d) None of them
60. London forces are also called:
🟥 a) Dipole-dipole force
🟦 b) van der Waals forces
🟩 c) Hydrogen bonding
🟨 d) All of them
61. The molar volume of CO₂ is maximum at:
🟥 a) STP
🟦 b) 127ºC and 1 atm
🟩 c) 0ºC and 2 atm
🟨 d) 273ºC and 2 atm
62. Equation used to determine density of a gas:
🟥 a) d = MP/RT
🟦 b) d = RT/MP
🟩 c) d = MRT
🟨 d) d = RP/MT
63. At constant pressure, at which temperature will volume of gas be twice of what it is at 0ºC?
🟥 a) 546ºC
🟦 b) 200ºC
🟩 c) 546 K
🟨 d) 273 K
64. If absolute temperature of a gas is doubled and pressure reduced to half, volume will:
🟥 a) Be doubled
🟦 b) Reduce to ¼
🟩 c) Remain unchanged
🟨 d) Quadruple
65. The temperature 273 K corresponds to:
🟥 a) 0ºC
🟦 b) 273ºC
🟩 c) 100ºC
🟨 d) –273ºC
66. Order of diffusion rate of NH₃, SO₂, Cl₂, CO₂:
🟥 a) NH₃ > SO₂ > Cl₂ > CO₂
🟦 b) NH₃ > CO₂ > SO₂ > Cl₂
🟩 c) NH₃ > CO₂ > Cl₂ > SO₂
🟨 d) Cl₂ > SO₂ > CO₂ > NH₃
67. Which pair of gases has same rate of diffusion?
🟥 a) Cl₂ and CO₂
🟦 b) C₃H₈ and CO₂
🟩 c) NH₃ and SO₂
🟨 d) Cl₂ and NH₃
68. Which gas has the slowest diffusion rate?
🟥 a) O₃
🟦 b) C₂H₂
🟩 c) C₂H₆
🟨 d) C₄H₁₀
69. Value of universal gas constant R is/are:
🟥 a) 8.3143 J·mol⁻¹·K⁻¹
🟦 b) 0.0821 atm·dm³·mol⁻¹·K⁻¹
🟩 c) 1.987 cal·mol⁻¹·K⁻¹
🟨 d) All of them
70. Which gas has the fastest diffusion rate?
🟥 a) O₂
🟦 b) C₂H₄
🟩 c) C₃H₆
🟨 d) C₄H₈
71. The compressibility factor for an ideal gas is:
🟥 a) 1.5
🟦 b) 1
🟩 c) 1
🟨 d) ∞
72. Pressure exerted by gas collected over water = 735 torr, dry gas = 705 torr. Aqueous tension is:
🟥 a) 1440 torr
🟦 b) 35 torr
🟩 c) 735 torr
🟨 d) 30 torr
73. Molecules of gas A travel 4× faster than gas B at same T. Ratio of molecular weights (MA/MB):
🟥 a) 4
🟦 b) ¼
🟩 c) 16
🟨 d) 1/16
74. Mixture of H₂ and O₂ in 2:1 volume diffuses through porous partition. Composition of gas coming out initially:
🟥 a) 1:2
🟦 b) 4:1
🟩 c) 1:4
🟨 d) 8:1
75. Which property has same value for H₂ and D₂ at same P and T?
🟥 a) Molecular mass
🟦 b) Average molecular speed
🟩 c) Average molecular K.E
🟨 d) Density
76. Pressure doubled, temperature halved simultaneously. Volume will be:
🟥 a) Same as before
🟦 b) ¼th as before
🟩 c) Twice as before
🟨 d) None
77. A pressure of 0.101325 bar in atmospheres is:
🟥 a) 0.01 atm
🟦 b) 1 atm
🟩 c) 0.1 atm
🟨 d) 10 atm
78. Under which conditions do real gases approach ideal behaviour?
🟥 a) 15 atm, 200 K
🟦 b) 15 atm, 500 K
🟩 c) 1 atm, 273 K
🟨 d) 0.5 atm, 500 K
79. According to kinetic theory at absolute zero temperature:
🟥 a) Molecular motion stops
🟦 b) Liquid helium freezes
🟩 c) Liquid hydrogen freezes
🟨 d) Water freezes
80. Boyle’s law is applicable in:
🟥 a) Isochoric process
🟦 b) Isobaric process
🟩 c) Isomeric process
🟨 d) Isothermal process
81. Densities of two gases are in ratio 1:16. Ratio of their diffusion rates is:
🟥 a) 1:16
🟦 b) 1:4
🟩 c) 16:1
🟨 d) 4:1
82. Dimensions of pressure are same as:
🟥 a) Energy
🟦 b) Force per unit volume
🟩 c) Mass per unit volume
🟨 d) Force per unit area
83. Atmospheric pressure experienced by human body is:
🟥 a) 14.7 psi
🟦 b) 14.7 torr
🟩 c) 0.95 atm
🟨 d) 2 Pa
84. Volume of gas at 30°C is X L. Volume becomes half at:
🟥 a) –121.5°C
🟦 b) 60°C
🟩 c) 15°C
🟨 d) None
85. Value of standard pressure in kilopascal is:
🟥 a) 1.01325 × 10²
🟦 b) 1.01325 × 10⁵
🟩 c) 1.01325 × 10⁶
🟨 d) 14.7
86. Molecules of gas A travel 8× faster than gas B at same T. Ratio of molecular weights (MA/MB):
🟥 a) 1/64
🟦 b) 1/32
🟩 c) 32
🟨 d) 64
87. Two spacecrafts: 10 m³ at 50 kPa, 30 m³ at 100 kPa. After connection, pressure is:
🟥 a) 150 kPa
🟦 b) 75 kPa
🟩 c) 87.5 kPa
🟨 d) 100 kPa
88. Coldest temperature at which all molecular motion ceases is:
🟥 a) –273.15°C
🟦 b) –459.7°C
🟩 c) 0 K
🟨 d) All of them
89. 100 ml H₂ effuses 4× faster than 100 ml unknown gas. Molecular weight of unknown gas:
🟥 a) 28 g
🟦 b) 64 g
🟩 c) 32 g
🟨 d) 80 g
90. Absolute temperature doubled, pressure increased 4×. Volume is:
🟥 a) Remains unchanged
🟦 b) Four times
🟩 c) Double
🟨 d) Half
91. The two gases which have the same molecular mass will have same:
🟥 a) Boiling point
🟦 b) Diffusion rate
🟩 c) Effusion rate
🟨 d) Both b and c
92. A gas is heated so that its volume halves and absolute temperature doubles. The pressure of the gas is:
🟥 a) Becomes half
🟦 b) Becomes 2 times
🟩 c) Becomes 4 times
🟨 d) Remains same
93. The value of universal gas constant depends upon:
🟥 a) Temperature of the gas
🟦 b) Volume of the gas
🟩 c) Number of moles of gas
🟨 d) None of these
94. Which process weakens the force of attraction between particles?
🟥 a) Evaporation
🟦 b) Freezing
🟩 c) Condensation
🟨 d) Crystallization
95. The relative rate of diffusion of H₂ and O₂ is:
🟥 a) 4:1
🟦 b) 1:4
🟩 c) 1:2
🟨 d) 1:8
96. Hydrogen gas diffuses 6 times faster than gas X. The molecular mass of X is:
🟥 a) 10
🟦 b) 72
🟩 c) 32
🟨 d) None of them
97. Heavy hydrogen (D₂) diffuses … times slower than H₂:
🟥 a) 1.41
🟦 b) 2
🟩 c) 4
🟨 d) 2.5
98. … law is helpful in separating different isotopes of a gas:
🟥 a) Graham’s law
🟦 b) Avogadro’s law
🟩 c) Dalton’s law
🟨 d) None
99. … is the weakest intermolecular force:
🟥 a) DDI
🟦 b) LDF
🟩 c) HBI
🟨 d) IDI
100. The molar volume of CO₂ is maximum at:
🟥 a) 227ºC and 1 atm
🟦 b) 0ºC and 2 atm
🟩 c) –273ºC and 2 atm
🟨 d) STP
✅ Answer Key with Short Reasons
1️⃣(Answer, d) 4:1 → Diffusion rate ∝ 1/√M; H₂ lighter than O₂.
2️⃣(Answer, b) Dalton’s law → Dry gas pressure = moist gas – water vapour pressure.
Collection of gas over water is an example of Dalton’s law. The pressure of dry gas is calculated by using Dalton’s law.
Pdry gas = Pmoist gas – Pwater vapours
3️⃣(Answer, c) 25°C & 1 atm → Higher T, lower P → maximum molar volume.
The molar volume of a gas varies directly with temperature and varies inversely with pressure. The molar volume of a gas is maximum at highest temperature and least pressure. In option c and d, temperature is highest hence deciding factor will be pressure which is least in option c.
4️⃣(Answer, b) 0 K → Absolute zero → theoretical zero volume.
The volume of gas would be theoretically zero at 0 K (-273°C).
5️⃣(Answer, d) Four times → V ∝ T/P; doubling T and halving P quadruples V.
PV=nRT ⇒ PV = T (R and n = constant) ⇒ V = T/P ⇒ V = 2/ ½ = 2 x 2 = 4
Thus, doubling the Kelvin temperature and halving the pressure quadruples the volume.
6️⃣(Answer, a) 0°C & 1 atm → STP conditions → 22.4 dm³ molar volume.
The molar volume of a gas is 22.4 dm3 at STP i.e. at 0°C and 1 atm.
7️⃣(Answer, b) 2 times → √(64/16) = 2; CH₄ diffuses twice as fast as SO₂.
8️⃣(Answer, d) Molar mass independent of T → Mass is constant, not affected by temperature.
9️⃣(Answer, c) Same molar mass (44 g/mol) → Equal diffusion rates.
The rate of diffusion depends upon molar masses of gases. The gases with same molar masses would have same rate of diffusion. The given gases ethane (C₃H₈) and CO₂ have same molar mass of 44 gmol⁻¹.
1️⃣0️⃣(Answer, d) High T & low P → Conditions where real gases behave ideally.
1️⃣1️⃣1:16 → Graham’s law: diffusion rate ∝ √(1/density). Ratio 4:1 → density ratio 1:16.
1️⃣2️⃣ → From rₓ/rᵧ = √(dᵧ/dₓ), solving gives dₓ = 12.
1️⃣3️⃣ 450 K → Using PV = nRT relation, calculation gives T₂ = 450 K.
1️⃣4️⃣ Positive deviation → Above Boyle temperature, compressibility factor Z > 1.
1️⃣5️⃣L/mol → b represents excluded volume per mole.
1️⃣6️⃣ Boyle temperature → Specific temperature where real gas obeys Boyle’s law.
1️⃣7️⃣ 1.863 → Z = PV/nRT; calculation gives ~1.863 (positive deviation).
1️⃣8️⃣ an²/V² → Corrects for intermolecular attractions in van der Waals equation.
1️⃣9️⃣Intermolecular attraction → a/V² term accounts for attractive forces.
2️⃣0️⃣ (P + a/V²) → Pressure correction term accounts for intermolecular forces.
2️⃣1️⃣ Remain constant → PV = constant is Boyle’s law, valid only at constant temperature.
2️⃣2️⃣ Doubled → KE ∝ T; doubling temperature doubles kinetic energy.
2️⃣3️⃣ Compressibility factor → PV/nRT = Z, measures deviation from ideal gas.
2️⃣4️⃣ 7.09 m³ → Volume per molecule = b/Nᴀ.
2️⃣5️⃣ 226.085 kPa → Conversion factor: 1 psi = 6.892 kPa.
2️⃣6️⃣ Depression → Meteorological term for low-pressure system.
2️⃣7️⃣ High temperature → Increases KE, reduces intermolecular attractions.
2️⃣8️⃣ 2 mole → 44.8 L ÷ 22.4 L/mol = 2 mol.
2️⃣9️⃣ Diffusion → Random spreading of molecules.
3️⃣0️⃣ Effusion → Escape through tiny hole into vacuum.
3️⃣1️⃣Elastic → Kinetic Molecular Theory: collisions of ideal gas molecules are perfectly elastic.
3️⃣2️⃣Equal to 1 → At zero pressure, compressibility factor Z → 1 (ideal behavior).
3️⃣3️⃣Low temperature → Lower KE → stronger intermolecular attractions.
3️⃣4️⃣NH₃ → Polar molecule with hydrogen bonding, not London forces.
3️⃣5️⃣General gas law → Combines Boyle’s and Charles’s laws into one expression.
3️⃣6️⃣Dalton’s law → Total pressure = sum of partial pressures of non-reacting gases.
3️⃣7️⃣Dalton’s law → Respiration involves partial pressures of gases in lungs/blood.
3️⃣8️⃣159.6 mm Hg → Partial pressure of oxygen in air at sea level.
3️⃣9️⃣Aqueous tension → Pressure due to water vapour in a gas mixture.
4️⃣0️⃣Gay-Lussac’s law → Volumes of gases in reactions combine in simple whole number ratios.
4️⃣1️⃣Pressure → Density formula d = PM/RT; directly proportional to pressure.
4️⃣2️⃣Temperature → Density inversely proportional to T in d=PM/RT.
4️⃣3️⃣200 ml/s → Graham’s law: CH₄ diffuses twice as fast as SO₂.
4️⃣4️⃣150 mm Hg → Oxygen partial pressure at altitude ~150 mm Hg causes discomfort.
4️⃣5️⃣Bond length → Isotopes have same nuclear charge → identical bond length.
4️⃣6️⃣Ideal gases → PV/nRT = 1 always → horizontal line.
4️⃣7️⃣Temperature → M = dRT/P → directly proportional to T.
4️⃣8️⃣M.W = RTd/P → Standard formula for molar mass using density.
4️⃣9️⃣Pressure → M inversely proportional to P in M = dRT/P.
5️⃣0️⃣Krypton → Noble gases are monoatomic.
5️⃣1️⃣ None of them → No real gas is perfectly ideal; ideal gas is hypothetical.
5️⃣2️⃣ All of them → All existing gases are real.
5️⃣3️⃣ Real gas → Deviates from gas laws at certain T and P.
5️⃣4️⃣ Low T, high P → Stronger intermolecular forces → non-ideal behavior.
5️⃣5️⃣ Non-polar gases → Weaker forces → more ideal.
5️⃣6️⃣ Polar gases → Stronger forces → more non-ideal.
5️⃣7️⃣ van der Waals forces → Short-range attractions between molecules.
5️⃣8️⃣ Temporary forces → van der Waals forces develop under low T, high P.
5️⃣9️⃣ London forces → Temporary dipoles in non-polar molecules/inert gases.
6️⃣0️⃣ van der Waals forces → London forces are a type of van der Waals force.
6️⃣1️⃣ 127ºC & 1 atm → High T, low P → maximum molar volume.
6️⃣2️⃣ d = MP/RT → Standard density formula.
6️⃣3️⃣546 K → Doubling absolute temperature doubles volume at constant pressure.
6️⃣4️⃣ Quadruple → Doubling T doubles V; halving P doubles V again → 4×.
6️⃣5️⃣ 0ºC → 273 K corresponds to 0ºC.
6️⃣6️⃣ NH₃ > CO₂ > SO₂ > Cl₂ → Diffusion rate inversely proportional to molar mass.
6️⃣6️⃣ C₃H₈ and CO₂ → Both have molar mass 44 g/mol → same diffusion rate.
6️⃣8️⃣ C₄H₁₀ → Highest molar mass → slowest diffusion.
6️⃣9️⃣ All of them → R has multiple equivalent values in different units.
7️⃣0️⃣ C₂H₄ → Lowest molar mass → fastest diffusion.
7️⃣1️⃣1 → Compressibility factor Z = PV/nRT; for ideal gas Z = 1.
7️⃣2️⃣30 torr → Aqueous tension = moist – dry = 735 – 705.
7️⃣3️⃣1/16 → Diffusion rate ∝ 1/√M; ratio gives MA/MB = 1/16.
7️⃣4️⃣8:1 → H₂ diffuses faster; composition ratio = 8:1.
7️⃣5️⃣Average KE → KE depends only on T, same for all gases.
7️⃣6️⃣Same as before → V ∝ T/P; halving T and doubling P cancels out.
7️⃣7️⃣0.1 atm → 0.101325 bar ≈ 0.1 atm.
7️⃣8️⃣0.5 atm, 500 K → High T, low P → ideal behaviour.
7️⃣9️⃣Motion stops → At absolute zero, molecular motion ceases.
8️⃣0️⃣Isothermal → Boyle’s law applies at constant T.
8️⃣1️⃣4:1 → Diffusion rate ratio = √16/√1 = 4:1.
8️⃣2️⃣Force per unit area → Pressure definition.
8️⃣3️⃣14.7 psi → Standard atmospheric pressure.
8️⃣4️⃣–121.5°C → Volume halves when T halves (Charles’s law).
8️⃣5️⃣1.01325 × 10² kPa → Standard pressure = 1 atm = 101.325 kPa.
8️⃣6️⃣1/64 → Diffusion rate ratio gives MA/MB = 1/64.
8️⃣7️⃣87.5 kPa → Weighted average pressure after connection.
8️⃣8️⃣All of them → –273.15°C, –459.7°F, 0 K all represent absolute zero.
8️⃣9️⃣32 g → Graham’s law calculation gives molar mass = 32 g.
9️⃣0️⃣Half → V ∝ T/P; doubling T and quadrupling P halves volume.
9️⃣1️⃣Both b and c → Diffusion/effusion rates depend only on molar mass; same mass → same rates.
9️⃣2️⃣4 times → P ∝ T/V; doubling T and halving V quadruples pressure.
9️⃣3️⃣None of these → R is universal constant; depends only on chosen units.
9️⃣4️⃣Evaporation → Converts liquid to gas, weakening intermolecular forces.
9️⃣5️⃣4:1 → Graham’s law: H₂ diffuses 4× faster than O₂.
9️⃣6️⃣72 → Graham’s law calculation gives molar mass of X = 72 g/mol.
9️⃣7️⃣1.41 → D₂ diffuses √2 times slower than H₂.
9️⃣8️⃣Graham’s law → Basis for isotope separation (lighter diffuses faster).
9️⃣9️⃣LDF → London dispersion forces are weakest intermolecular forces.
1️⃣0️⃣0️⃣227ºC & 1 atm → High T and low P → maximum molar volume.
🧠
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