MDCAT/ECAT/FSC Chapter-wise High-Yield Chemistry MCQs on Gaseous State

👋 Assalamualaikum & Welcome Learners!

Welcome to InamJazbi Learn Chemistry! 💡 I’m Inam Jazbi, and you’re now learning chemistry with InamJazbi Learn Chemistry — your trusted platform for MDCAT & ECAT high-yield preparation.

🎓 Here you’ll find MDCAT & ECAT focused high-yield chemistry MCQs specially curated to boost your exam score. 💯 Practice, revise, and master the Gaseous State with ease.

🔥 This quiz covers TOP most repeated MCQs on the Gaseous State specially designed to:

✔ Boost your MDCAT/ECAT score

✔ Strengthen your concepts of KMT, gas laws like Boyle’s law, Charles’s law, Graham’s law, Daltons, Law, general gas equation, van der Waal’s equation etc.

✔ Improve accuracy & speed in solving exam-style questions

✔ Prepare you like a real exam with instant feedback

Let’s make chemistry simple, fun, and rewarding! 🚀

💥 MDCAT / ECAT Chemistry Chapter‑wise High‑Yield 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 (Mᴀ/Mʙ):

🟥 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 (Mᴀ/Mʙ):

🟥 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.

r₁/r₂= √M₂/√M₁ ⇒ r₁/r₂= √32/√2 ⇒ r₁/r₂= √16 ⇒ r₁/r₂= 4:1

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.

r₁/r₂ = √M₂/√M₁ ⇒ r₁/r₂ = √64/√16 ⇒ r₁/r₂ = √4 ⇒ r₁/r₂ = 2

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.

🧠 Related Posts:

https://learnchemistrybyinamjazbi.blogspot.com/2025/12/mcqs-quiz-chemical-bonding-for-mdcat.html

MCQs Quiz Chemical Bonding for MDCAT, ECAT & FSC: Your Ultimate Practice Guide!

https://learnchemistrybyinamjazbi.blogspot.com/2025/12/mdcatecatfsc-chapter-wise-high-yield.html

MDCAT/ECAT/FSC Chapter-wise High-Yield Chemistry MCQs Quiz on Atomic Structure

🔥🌟 جونؔ ایلیا 🔥🌟

🔥💥 جونؔ ایلیا کے اشعار 🔥💥

📖 حال خوش تذکرہ نگاروں کا
🏙️ تھا تو اک شہر خاکساروں کا
🏠 پہلے رہتے تھے کوچۂ دل میں
💔 اب پتہ کیا ہے دل فگاروں کا
🚫 کوئے جاناں کی ناکہ بندی ہے
🛏️ بسترا اب کہاں ہے یاروں کا
🌬️ چلتا جاتا ہے سانس کا لشکر
🕯️ کون پُرساں ہے یادگاروں کا
🤦‍♂️ اپنے اندر گھسٹ رہا ہوں میں
❓ مجھ سے کیا ذکر رہ گزاروں کا
👥 ان سے جو شہر میں ہیں بے دعویٰ
🎉 عیش مت پوچھ دعویداروں کا
⚔️ کیسا یہ معرکہ ہے برپا جو
🐎 نہ پیادوں کا نہ سواروں کا
🗣️ بات تشبیہہ کی نہ کیجیو تُو
🔮 دہر ہے صرف استعاروں کا
🕊️ میں تو خیر اپنی جان ہی سے گیا
🤷‍♂️ کیا ہوا جانے جانثاروں کا
🔥 کچھ نہیں اب سوائے خاکستر
🔥 ایک جلسہ تھا شعلہ خواروں کا

😏 ہر طنز کیا جائے ہر اک طعنہ دیا جائے
🚫 کچھ بھی ہو پر اب حد ادب میں نہ رہا جائے
📜 تاریخ نے قوموں کو دیا ہے یہی پیغام
✊ حق مانگنا توہین ہے حق چھین لیا جائے

🌌 ؎ خلد گم گشتہ کا موضوع نہ چھیڑو کہ مجھے
🩸 اپنے خوں گشتہ خیالوں سے حجاب آتا ہے
🧠 یادِ ماضی سے میرے ذہن کو محفوظ رکھو
⚡ یاد ماضی نہیں آتی ہے عذاب آتا ہے

⏳ لمحہ لمحہ پڑھا کرے انسان
🕯️ نوحہ کل من علیہا فانٍ

🔥💥 جونؔ ایلیا کے اشعار 🔥💥

🚫 ؎ انکار ہے تو قیمت انکار کچھ بھی ہو
⚡ یزداں سے پوچھنا یہ ادا اہرمن میں تھی

🤯 میں بھی بہت عجیب ہوں اتنا عجیب ہوں کہ بس
💔 خود کو تباہ کر لیا اور ملال بھی نہیں

⏳ جو گزاری نہ جا سکی ہم سے
📖 ہم نے وہ زندگی گزاری ہے

😔 یہ مجھے چین کیوں نہیں پڑتا
🧑‍🤝‍🧑 ایک ہی شخص تھا جہان میں کیا

🌹 کتنی دل کش ہو تم کتنا دلجو ہوں میں
⚰️ کیا ستم ہے کہ ہم لوگ مر جائیں گے

🏚️ کون اس گھر کی دیکھ بھال کرے
🪞 روز اک چیز ٹوٹ جاتی ہے

🤷‍♂️ کیسے کہیں کہ تجھ کو بھی ہم سے ہے واسطہ کوئی
🤐 تو نے تو ہم سے آج تک کوئی گلہ نہیں کیا

💞 کیا کہا عشق جاودانی ہے!
🕰️ آخری بار مل رہی ہو کیا

🔥💥 جونؔ ایلیا کے اشعار 🔥💥

🏘️ اس گلی نے یہ سن کے صبر کیا
🚶‍♂️ جانے والے یہاں کے تھے ہی نہیں

🌍 حاصل کن ہے یہ جہان خراب
⏳ یہی ممکن تھا اتنی عجلت میں

⚔️ یہ وار کر گیا ہے پہلو سے کون مجھ پر
🔄 تھا میں ہی دائیں بائیں اور میں ہی درمیاں تھا

🌫️ ساری گلی سنسان پڑی تھی باد فنا کے پہرے میں
👤 ہجر کے دالان اور آنگن میں بس اک سایہ زندہ تھا

🔄 اک عجب آمد و شد ہے کہ نہ ماضی ہے نہ حال
📜 جونؔ برپا کئی نسلوں کا سفر ہے مجھ میں

🏰 حملہ ہے چار سو در و دیوار شہر کا
🌳 سب جنگلوں کو شہر کے اندر سمیٹ لو

🏠 پہلے رہتے تھے کوچئہ دل میں
💔 اب پتا کیا ہے دل فگاروں کا جونؔ

🔥 جونؔ ایلیا کے اشعار 🔥

😔 یہ مجھے چین کیوں نہیں پڑتا
🧑‍🤝‍🧑 ایک ہی شخص تھا جہان میں کیا

🌹 کتنی دل کش ہو تم کتنا دلجو ہوں میں
⚰️ کیا ستم ہے کہ ہم لوگ مر جائیں گے

🏚️ کون اس گھر کی دیکھ بھال کرے
🪞 روز اک چیز ٹوٹ جاتی ہے

🤲 بہت نزدیک آتی جا رہی ہو
💔 بچھڑنے کا ارادہ کر لیا کیا

🤷‍♂️ کیسے کہیں کہ تجھ کو بھی ہم سے ہے واسطہ کوئی
🤐 تو نے تو ہم سے آج تک کوئی گلہ نہیں کیا

💞 کیا کہا عشق جاودانی ہے!
🕰️ آخری بار مل رہی ہو کیا

🪨 علاج یہ ہے کہ مجبور کر دیا جاؤں
🙉 وگرنہ یوں تو کسی کی نہیں سنی میں نے

🏘️ اس گلی نے یہ سن کے صبر کیا
🚶‍♂️ جانے والے یہاں کے تھے ہی نہیں

🌍 حاصل کن ہے یہ جہان خراب
⏳ یہی ممکن تھا اتنی عجلت میں

🔗 اب جو رشتوں میں بندھا ہوں تو کھلا ہے مجھ پر
🕊️ کب پرند اڑ نہیں پاتے ہیں پروں کے ہوتے

🔥 جونؔ ایلیا کے اشعار 🔥

🏠 آج بہت دن بعد میں اپنے کمرے تک آ نکلا تھا
🌸 جوں ہی دروازہ کھولا ہے اس کی خوشبو آئی ہے

⚔️ یہ وار کر گیا ہے پہلو سے کون مجھ پر
🔄 تھا میں ہی دائیں بائیں اور میں ہی درمیاں تھا

🌫️ ساری گلی سنسان پڑی تھی باد فنا کے پہرے میں
👤 ہجر کے دالان اور آنگن میں بس اک سایہ زندہ تھا

🔄 اک عجب آمد و شد ہے کہ نہ ماضی ہے نہ حال
📜 جونؔ برپا کئی نسلوں کا سفر ہے مجھ میں

🏰 حملہ ہے چار سو در و دیوار شہر کا
🌳 سب جنگلوں کو شہر کے اندر سمیٹ لو

🏠 پہلے رہتے تھے کوچئہ دل میں
💔 اب پتا کیا ہے دل فگاروں کا جونؔ

⚠️ کیا کہوں جان کو بچانے میں
☠️ جونؔ خطرہ ہے جان جانے کا
🔥 یہ جہاں جونؔ! اک جہنم ہے
🚫 یاں خدا بھے نہیں ہے آنے کا
⏳ زندگی ایک فن ہے لمحوں کا
🎭 اپنے انداز سے گنوانے کا

🌙 آج کے بعد عشرتِ مجلسِ شامِ غم کہاں
💔 دل نہ لگے گا تیرے بعد پر تیرے بعد ہم کہاں
🌸 نکہتِ یاسمین قبا بھول نہ جائیو ہمیں
🌅 صبح کے بعد تُو کہاں شام کے بعد ہم کہاں
😶 یہ جو نواگری کے ساتھ چیخ نہیں رہا ہوں میں
🫀 سینہ نے نواز میں آخر اب اتنا دم کہاں
👁️ اب یہ جبین و چشم و لب تجھ کو نظر نہ آئیں گے
🔍 غور سے دیکھ لے ہمیں آج کے بعد ہم کہاں