Here is a vast collection of objective and subjective questions in this question bank of **chemistry 11, chapter 03**. Following types of questions have been included here.

**MCQs (Textbook Exercise)****MCQs (Previous Boards Essentials)****SQs Topic-wise (Previous Boards Essentials + Textbook Conceptuals)****LQs (Previous Boards Essentials)**

You can find solutions to these questions from our publication, **“An Insight Into Objective Chemistry-11”.**

**MCQs (Textbook Exercise)**

**Q. Each question has four possible answers. Tick the correct one.**

**01: Pressure remaining constant at which temperature the volume of a gas will become twice of what it is at 0 ^{o}C: (BWP-18,19)(GJR-19,19)(SRG-19,19)(FSL-19,21)(RWP-19,21,22,23)(SWL-19,23)(DGK-22,23)(LHR-23)(MLT-23)**

(a) 546^{o}C

(b) 200^{o}C

(c) 546 K

(d) 273 K

**02: Number of molecules in one dm ^{3} of water is close to: (LHR-16)(DGK-16)(AJK-16,19)(SRG-17,19)(BWP-18)(RWP-18)**

(a) 6.02/22.4 ⤫ 10^{23}

(b) 12.04/22.4 ⤫ 10^{23}

(c) 18/22.4 ⤫ 10^{23}

(d) 55.6 × 6.02 ⤫ 10^{23}

**03: Which of the following, will have the same number of molecules at STP? (BWP-22)(LHR-22,22)**

(a) 280 cm^{3} of CO_{2} and 280 cm^{3} of N_{2}O

(b) 11.2 dm^{3} of O_{2} and 32 g of O_{2}

(c) 44 g of CO_{2} and 11.2 dm^{3} of CO

(d) 28 g of N_{2} and 5.6 dm^{3} of oxygen

**04: If absolute temperature of a gas is doubled and the pressure is reduced to one half, the volume of the gas will be: (LHR-17)(MLT-17,21)(DGK-18)(BWP-18)(GJR-19)**

(a) Remain unchanged

(b) Increase four times

(c) Reduce to 1/4

(d) Be doubled

**05: How should the conditions be changed to prevent the volume of a given gas form expanding when it’s mass is increased? (LHR-22)(DGK-22)**

(a) Temperature is lowered & pressure is increased.

(b) Temperature is increased & pressure is lowered.

(c) Temperature and pressure both are lowered.

(d) Temperature and pressure both are increased.

**06: The molar volume of CO _{2} is maximum at: **

**(DGK-16)(SRG-18)(GJR-18,19,22,22)(AJK-16)(BWP-16,17,18,19,21)(RWP-17,17)(LHR-19,22)(MLT-19)(SWL-19)(FSL-19,19)**

(a) STP

(b) 127^{o}C and 1 atm

(c) 0^{o}C and 2 atm

(d) 273^{o}C and 2 atm

**07: The order of the rate of diffusion of gasses NH _{3}, SO_{2}, Cl_{2} and CO_{2} is: **

**(FSL-17)(BWP-17)(SRG-17,18,23)(MLT-17,19)(RWP-18,22)(LHR-19)(AJK-19)(DGK-22,23)**

(a) NH_{3}>SO_{2}>Cl_{2}>CO_{2}

(b) NH_{3}>CO_{2}>SO_{2}>Cl_{2}

(c) Cl_{2}>SO_{2} CO_{2}>NH_{3}

(d) NH_{3}>CO_{2}>Cl_{2}>SO_{2}

**08: Equal masses of CH _{4} and oxygen are mixed in an empty container at 25^{o}C. The fraction of total pressure exerted by oxygen is: (LHR-17,18)(FSL-17,18,21,23)(GJR-17,21,22)(SRG-18,19)(DGK-21)(BWP-21,22)SWL-22)**

(a) 1/3

(b) 8/9

(c) 1/9

(d) 16/17

**09: Gases deviate from ideal behavior at high pressure. Which of the followings is correct for non-ideality? (FSL-22)**

(a) At high pressure, the gas molecules move in one direction only.

(b) At high pressure, the collisions between the gas molecules are increased manifold.

(c) At high pressure, the volume of the gas becomes insignificant.

(d) At high pressure, the intermolecular attractions become significant.

**10: The deviation of gas form ideal behavior is maximum at: (RWP-17)(AJK-17)(LHR-17,19)(DGK-17,19,22)(FSL-18,22)(BWP-19,23)(MLT-19,23)(SWL-22)**

(a) –10^{o}C and 5.0 atm

(b) –10^{o}C and 2.0 atm

(c) 100^{o}C and 2.0 atm

(d) 0^{o}C and 2.0 atm

**11: A real gas obeying van der Waals equation will resemble ideal gas if: (SWL-17)(GJR-17)(MLT-17,19)(BWP-19)(FSL-19,23)**

(a) Both “a” and “b” are large

(b) Both “a” and “b” are small

(c) “a” is small and “b” is large

(d) “a” is large and “b” is small

**MCQs (Previous Boards Essentials)**

**Q. Each question has four possible answers. Tick the correct one.**

**01: The SI unit of pressure is: (DGK-17,19)(MLT-18)(BWP-23**)

(a) Nm^{-1 }

(b) Nm^{-2 }

(c) Nm^{‑3}

(d) mm Hg

**02: 1 atmosphere is equal to: (FSL-23)**

(a) 760 mm of Hg

(b) 1000 mm of Hg

(c) 760 cm of Hg

(d) 20 Psi

**03: The commonly used unit of pressure by meteorologists is: (AJK-17)**

(a) Atmosphere

(b) Pascal

(c) Millibar

(d) psi

**04: The unit millibar is commonly used by: (LHR-19) **

(a) Meteorologists

(b) Astronauts

(c) Engineers

(d) Dalton

**05: Temperature and number of moles are kept constant in: (DGK-21)(BWP-23)**

(a) Boyle’s law

(b) Charles’s law

(c) Avogadro’s law

(d) Dalton’s law of partial pressures

**06: Graph between pressure and volume at constant temperature is called: (BWP-23)**

(a) Isobar

(b) Isochor

(c) Isotherm

(d) Spectrograph

**07: Constant factor in Charles’ law: (SRG-23)**

(a) Volume

(b) Pressure

(c) Temperature

(d) Both V and T

**08: The value of ‘R’ in Nm K ^{-1 }mol^{-1} is: (FSL-23) **

(a) 1.987

(b) 8.3143

(c) 0.0821

(d) 2.4

**09: At absolute zero, total kinetic energy of gas molecules is: (MLT-21)**

(a) Maximum

(b) Zero

(c) Never becomes lower than 20 K

(d) Minimum

**10: The density of gas can be determined by the formula: (LHR-21)(SWL-21,23)**

(a) d=PM/RT

(b) d=RT/PM

(c) d=PMR/T

(d) d=PMT/R

**11: Mass of 22.414 dm ^{3} of N_{2} at STP is: (BWP-17) **

(a) 28 g

(b) 14 g

(c) 1.4 g

(d) 2.8 g

**12: Dalton’s law of partial pressures can be derived from: (MLT-21) **

(a) Avogadro’s law

(b) General gas equation

(c) Charles’s law

(d) All of these

**13: The partial pressure of oxygen in air is:** **(SRG-17)(DGK-23)(GJR-23)(LHR-23)**

(a) 156 torr_{ }

(b) 157 torr _{}

(c) 158 torr

(d) 159 torr

**14: Partial pressure of oxygen in human lungs in torr is: (LHR-17)(RWP-21) **_{}

(a) 161 torr_{ }

(b) 116 torr

(c) 159 torr

(d) 760 torr

**15: Which of the following will have highest rate of diffusion? (SWL-17)**

(a) CO_{2 }

(b) NH_{3 }

(c) HCl

(d) SO_{2}

**16: The spreading of fragrance of a rose or scent in air is due to: (SWL-18)**

(a) Effusion

(b) Diffusion

(c) Osmosis

(d) Evaporation

**17: The kinetic equation was derived by: (MLT-21) **

(a) Maxwell

(b) Boltzmann

(c) Clausius

(d) Bernoulli

**18: The highest temperature at which a substance can exist as liquid state at its critical temperature is: (DGK-19)**

(a) Absolute zero

(b) Consulate temperature

(c) Critical temperature

(d) Transition temperature

**19: Critical temperature of water vapours is: (DGK-23) **

(a) 647.6K (b) 405.6K (c) 546K (d) 273K

**20: Critical temperature of NH _{3} is: (BWP-16) **

(a) 132.44^{o}C

(b) –132.44^{o}C

(c) 0^{o}C

(d) 136.25^{o}C

**21: All gases can be liquified by Linde’s method except: (LHR-23)**

(a) N_{2}

(b) O_{2}

(c) F_{2}

(d) He

**22: The scientist who identified plasma: (RWP-23)**

(a) William Crooks

(b) Van der Waals’

(c) Rutherford

(d) Boyle

**23: The sun is a ________ kilometer ball of plasma heated by nuclear fusion. (MLT-21) **

(a) 1.5 million kilometer

(b) 1.5 billion kilometer

(c) 3 million kilometer

(d) None of these

**24: The temperature of natural plasma is about: (DGK-17)(FSL-22)**

(a) 20,000^{o}C

(b) 10,000^{o}C

(c) 5000^{o}C

(d) 1000^{o}C

**SHORT QUESTIONS**

**3.1: STATES OF MATTER**

**Q.01: **What are the states of matter?

**Q.02: **Why are liquids less common than other forms of matter?

**Q.03: **Write any four properties of liquids. **(SRG-19)**

**Q.04: **What is one atmosphere pressure? **(SRG-19)**

**Q.05: **Define pressure. Give its two units? **(FSL-23)**

**3.2: GAS LAWS**

**Q.06: **Define gas laws.

**Q.07: **State Boyle’s law and write its mathematical form.** (MLT-21)(BWP-22,23)**

**Q.08: **What do you mean by the term isotherm?** (DGK-21)(RWP-21) **

**Q.09: **What happens to the positions of isotherms, when they are plotted at higher temperatures? OR Why does the graph plotted between pressure and volume move away from pressure axis at higher temperature? **(DGK-21)(LHR-21)**

**Q.10: **Why does the graph between P and 1/V give straight line? What is the effect of temperature on the position of this straight line? **(LHR-19)**

**Q.11: **The graph between P and PV is a straight line. Explain why?** (LHR-16)(GJR-18)**

**Q.12: **Explain that value of k in Boyle’s law depends on: (a) Temperature (b) Quantity of gas.

**Q.13: **State Charles’s law. Write its mathematical form.** (SRG-19)(GJR-21)(MLT-21)(FSL-22,23)**

**Q.14: **Write down the quantitative definition of Charles’s law.

**(LHR-21)(RWP-21)(SWL-21)(FSL-22)(GJR-23)**

**Q.15: **Justify that the volume of given mass of a gas becomes theoretically zero at –273^{o}C.

**Q.16: **Throw some light on the factor 1/273 in Charles’s law.** (RWP-17)(BWP-19)(SRG-23)**

**Q.17: **Define absolute Zero.** (FSL-16,19)(LHR-16,17)(DGK-17)(SRG-19)(SRG-22)**

**Q.18: **What is absolute zero? Show it by drawing a graph.** (DGK-19)**

**Q.19: **How is absolute zero explained by drawing graph?** (MLT-19)(FSL-23)**

**Q.20: **Do you think that the volume of any quantity of a gas becomes zero at –273.16^{o}C? Is it not against the law of conservation of mass?

**Q.21: **Absolute zero (–273.15^{o}C) is the lowest possible (coldest) temperature. Give reason.** (SWL-19)**

**Q.22: **Describe different scales of thermometry. OR What is centigrade scale of thermometry. **(FSL-21,21)**

**Q.23: **Write formulas for interconversion of various scales of temperature.** (DGK-21)(LHR-22)**

**Q.24: **Convert: (a) –40^{o}F into Centigrade scale. (b) 40^{o}C into Fahrenheit scale. **(RWP-16,19)(FSL-16)(BWP-19)(GJR-22)**

**Q.25: **Convert 30^{o }to Fahrenheit scale. **(RWP-22)**

**3.3: GENERAL GAS EQUATION**

**Q.26: **Briefly discuss/derive general gas equation.** (FSL-21)(MLT-21)**

**Q.27: **What is R? What is its physical significance?** (GJR-21)(LHR-21)**

**Q.28: **Calculate the value of R at STP. OR Derive the units of ‘R’ when pressure is in atmosphere and volume is in dm^{3}. **(BWP-16)(LHR-18)(FSL-21,22)**

**Q.29: **Calculate the value of R in SI units.** (MLT-16,17,19,21,21)(LHR-16,19,21)(FSL-17,18,19)(SRG-17,19)(DGK-17,21)(GJR-19,21,23)(BWP-19)(SWL-21,23)**

**Q.30: **Drive the values of ‘R’ when the pressure is in Nm^{–1 }and Volume in m^{3}.** (SWL-22)(DGK-23)**

**Q.31: **Derive mathematical relationship for density of an ideal gas.** (LHR-23)**

**Q.32: **How the densities of ideal gases can be calculated from ideal gas equation?** (LHR-22)**

**Q.33: **Derive formula to determine the density of a gas from ideal gas equation.

**Q.34: **How is the density of gas related to temperature and pressure of the gas?

**Q.35: **Prove that d = PM/RT.** (RWP-16)(LHR-17)(DGK-17,21,22)(SRG-19)(BWP-19)(MLT-21)(SWL-23)**

**Q.36: **Why do we feel comfortable in expressing the densities of gases in units of g dm^{3} rather than g cm^{3}? **(MLT-23)**

**Q.37: **Why are the densities of gases expressed in the units of g dm^{–3}, while that of liquids and solids are expressed in unitsof g cm^{–3}?** (DGK-16)(LHR-17)**

**3.4: AVOGADRO’S LAW**

**Q.38: **What is Avogadro’s law of gases? Give example.** (LHR-23)**

**Q.39: **State Avogadro’s law. **(DGK-16,17)(LHR-16,21)**

**(GJR-17,21,23)(FSL-18)(BWP-18)(SWL-19,21,22,23)(SRG-19)(MLT-21)(RWP-22) **

**Q.40: **Justify that 1cm^{3 }of H_{2} and 1 cm^{3} of CH_{4} at STP will have same number of molecules, when one molecule of CH_{4} is 8 times heavier than that of H_{2}.** (MLT-23)**

**Q.41: **Do you think that 1 mole of H_{2} and 1 mole of NH_{3} at 0^{o}C and 1 atm pressure will have Avogadro’s number of particles? **(GJR-15,18)**

**3.5: DALTON’S LAW OF PARTIAL PRESSURES**

**Q.42: **State Dalton’s law of partial pressures. Give its expression.** (FSL-19)(DGK-21)(MLT-21)**

**Q.43: **Define partial pressure. **(RWP-21)**

**Q.44: **Dalton’s law of partial pressures is only obeyed by those gases which do not have any attractive forces among their molecules. Explain.

**Q.45: **How does Dalton’s law help in calculating the pressure of gas collected over water? OR What is aqueous tension? OR How pressure of a dry gas can be calculated?**(MLT-16)(GJR-21)**

**Q.46: **What is aqueous tension? How you can find pressure of a gas over water in a container? **(DGK-23)**

**Q.47: **How does Dalton’s law explain the process of respiration? **(RWP-19)(SWL-22)(GJR-23)**

**Q.48: **At higher altitude, pilots feel uncomfortable breathing, why? OR Why do pilots use pressurized cabin?** (SRG-17)(SWL-18)(RWP-18,22)(DGK-19,21)(LHR-21,23)**

**Q.49: **Deep sea divers or scuba divers do not use normal air in breathing, why?** (DGK-17)(RWP-16)(SRG-17)(AJK-17)**

**Q.50: **Why normal air cannot be used in divers’ tank?** (DGK-22)(SWL-23)**

**Q.51: **Write down any two applications of Dalton’s law of partial pressures.** (AJK-19)(FSL-21)**

**3.6: DIFFUSION AND EFFUSION**

**Q.52: **Define diffusion and effusion of gases. **(MLT-19)**

**Q.53: **Define diffusion?** (BWP-22)**

**Q.54: **Differentiate between diffusion and effusion. **(BWP-17,18,22)(AJK-17)(SWL-17)(MLT-17)(RWP-17)(FSL-18)(DGK-22)(LHR-23)**

**Q.55: **State Graham’s law of diffusion. Give its mathematical expression. **(MLT-16)(BWP-17)(GJR-19)(DGK-19,19)**

**Q.56: **Lighter gases diffuse more rapidly than heavier gases. Give reason. **(DGK-15,19)(LHR-16,19)(RWP-17)(MLT-19)(BWP-19)**

**Q.57: **Why rate of diffusion of NH_{3} is more than HCl gas?** (BWP-23)**

**3.7: KINETIC MOLECULAR THEORY OF GASES****.**

**Q.58: **List the four postulates of kinetic molecular theory of gases.** (SRG-23)**

**Q.59: **Describe law of distribution of velocities. **(FSL-21)**

**Q.60: **Define mean square velocity and root mean square velocity.

**Q.61: **Differentiate between mean square velocity and root mean square velocity.

**Q.62: **Write expression for kinetic equation and root mean square velocity of gases.** (MLT-19) **

**Q.63: **Derive Boyle’s law from KMT.** (DGK-18,23)(GJR-19,21)(MLT-19)(LHR-21)(BWP-23)**

**Q.64: **Derive Charles’s law from KMT.** (RWP-19)(BWP19)(LHR-22) **

**Q.65: **Derive Avogadro’s law from KMT.** (MLT-18,19)(AJK-19)(FSL-21)**

**Q.66: **Derive Graham’s law of diffusion from kinetic equation.** (LHR-21)**

**3.8: KINETIC INTERPRETATION OF TEMPERATURE**

**Q.67: **How does heat flow from hotter to colder body?

**3.9: LIQUEFACTION OF GASES**

**Q.68: **Define critical temperature. On what factors does it depend?** (SWL-23)**

**Q.69: **Define critical temperature (T_{c}) with one example.** (AJK-19)(BWP-22)**

**Q.70: **Define critical temperature and critical pressure of a substance.** (FSL-22)**

**Q.71: **Define critical temperature, critical pressure, and critical volume.** (DGK-16,17)(LHR-16)(MLT-17,18)(BWP-17)(GJR-19,19)(FSL-19)**

**Q.72: **What is critical temperature and pressure of gas? Write name and formula of a gas whose critical temperature is above room temperature.** (DGK-19)**

**Q.73: **What is critical temperature of a gas? What is its importance for liquefaction of gases? **(BWP-23)**

**Q.74: **How is the critical temperature an essential criterion to be considered for the liquefaction of gases? Or What is the importance of critical temperature for liquefaction of gases?

**Q.75: **Polar gases have higher critical temperature than non-polar gases. Why?

**Q.76: **Define and explain Joule-Thomson effect. **(FSL-17,19,22)(MLT-17,18,19)(LHR-19)(RWP-22)**

**Q.77: **Give general principle of liquefaction of gases. **(FSL-19)**

**Q.78: **Why H_{2} and He cannot be liquefied by Linde’s method?** (FSL-19)**

**3.10: NON-IDEAL BEHAVIOUR OF GASES**

**Q.79: **Define compressibility factor.

**Q.80: **Differentiate between an ideal and a real gas.

**Q.81: **Why do real gases deviate from ideal behavior?** (SWL19)(DGK-22)**

**Q.82: **What are the causes of deviation of real gases from ideality?** (LHR-23)**

**Q.83: **Give two causes of deviation of real gases from ideal behavior. OR Real gases show non-ideal behaviour due to two assumptions of kinetic molecular theory, explain. **(SWL-18)(LHR-19)(FSL-16)(BWP-17,17)(DGK-19,23)**

**Q.84: **What are two faulty points of kinetic molecular theory of gases.** (GJR-19)(LHR-22)(RWP-23)**

**Q.85: **Gases show non-ideal behaviour at low temperature and high pressure, give reason. **(LHR-23)**

**Q.86: **Why do gases deviate from ideal behaviour at high pressure and low temperature? **(DGK-16,22)(BWP-17)(FSL-17)(MLT-18)(GJR-19)(RWP-23)**

**Q.87: **Gases deviate from ideal behaviour more at 0^{o}C than at 100^{o}C. Give the reason.** (DGK-23)**

**Q.88: **What is the effect of pressure and heat on the behaviour of gases?** (GJR-23)**

**Q.89: **Why do polar gases deviate more from ideality than non-polar gases?

**Q.90: **Water vapours don’t behave ideally at 273 K. **(GJR-17,18)(DGK-16,17)(MLT-18,23)(SRG-19)(LHR-22)(GJR-22)**

**Q.91: **SO_{2 }is comparatively non-ideal at 273 K but behaves ideally at 373 K. **(BWP-16,18)(RWP-17)(SRG-17)(GJR-17)(DGK-18)**

**Q.92: **H_{2} and He are ideal at room temperature but SO_{2 }and Cl_{2 }are non-ideal Explain. **(GJR-18)(SRG-18)**

**Q.93: **Why was volume correction done by van der Waals?

**Q.94: **What is b? Why is it greater than the actual volume of the gas molecules?

**Q.95: **Why was the pressure correction done by van der Waals’?

**Q.96: **The pressure of NH_{3} gas at given condition (say 20 atm pressure and room temperature) is less when calculated by van der Waals equation than that calculated by general gas equation, why?

**Q.97: **What are van der Waal’s constants? What is their physical significance?** **

**Q.98: **What is the physical significance of van der Waal’s constants ‘a’ and ‘b’? give their units. **(FSL-23,23)**

**Q.99: **What are the units of ‘a’ and ‘b’? **(MLT-18) **

**Q.100: **Derive the SI units of van der Waal’s constant.** (LHR-19)(BWP-19)**

**3.11: PLASMA STATE**

**Q.101: **What is plasma? **(FSL-14)**

**Q.102: **Define plasma. How is it formed? **(GJR-19)(RWP-23)**

**Q.103: **How plasma is formed? **(BWP-22)**

**Q.104: **Define plasma. Why is it neutral? **(BWP-19)**

**Q.105: **Define plasma. Also give its application. **(BWP-19)**

**Q.106: **What are natural and artificial plasma? OR What are the types of plasma? **(MLT-16)(BWP-16,23)(FSL-18,22)**

**Q.107: **What is the difference between natural and artificial plasma?** (DGK-23)**

**Q.108: **Where is plasma found? **(GJR-21)(GJR-23)**

**Q.109: **What are the characteristics of plasma? OR Write down two characteristics of plasma. **(BWP-17,18)(LHR-18,19,21,21)(SWL-19,23)(DGK-21)(GJR-21)(FSL-21)(RWP-22)(SRG-23)**

**Q.110: **Give important uses of plasma. OR Write any two applications of plasma. **(MLT-16,17)(AJK-16,19)(DGK-16,19,21,22)(LHR-17)(SRG-17)(FSL-17,18,19,23)(BWP-23)****Q.111: **What is future horizon of plasma? **(SWL-21)**

**LONG QUESTIONS**

**3****.2: GAS LAWS**

**01: **State Boyle’s law. Give its experimental verification. **(MLT-21)**

**02: **State Charles’s law. Explain its experimental verification. **(LHR-21)**

**03: **A gas having a volume of 10 dm^{3 }is enclosed in a vessel at 0^{o}C and the pressure is 2.5 atm. This gas is allowed to expand until the new pressure is 2 atm. What will be the new volume of this gas, if the temperature is maintained at 273K. **(SWL-22)**

**04: **250 cm^{3} of hydrogen is cooled from 127^{o}C to –27^{o}C by maintaining the pressure constant. Calculate the new volume of gas at constant temperature. **(GJR-19,22)(FSL-19,22)(RWP-22)(DGK-23)**

**3****.****3****: GENERAL GAS EQUATION**

**05: **Derive general gas equation for one mole of a gas from gas laws at STP. **(FSL-21)**

**06: **State and explain general gas equation. Calculate value of ‘R’ in SI units. **(DGK-17)(LHR-17)**

**07: **What is ideal gas constant ‘R’? Calculate its values in different units. **(BWP-16)(SRG-17)**

**08: **Derive an expression from general gas equation to calculate the density of gas. **(DGK-16)**

**09: **A sample of nitrogen gas is enclosed in a vessel of volume 380 cm^{3} at 120°C and pressure of 101325 Nm^{-2}. This gas is transferred to a 10 dm^{3} flask and cooled to 127^{o}C. Calculate the pressure in Nm^{-2} exerted by the gas at 27°C. **(SRG-19)(LHR-19,22,23)(DGK-22)**

**10: **Calculate the density of CH_{4} at 0^{o}C and 1 atmosphere pressure. **(FSL-19)(DGK-19)(BWP-19)(AJK-19)**

**11: **Calculate the density of CH_{4} at 0^{o}C and 1 atmosphere pressure. What happened to the density if pressure increased to 2atm at 0^{o}C? **(GJR-22)**

**12: **Calculate the density of CH_{4} at 0^{o}C and 1 atmosphere pressure. What happened to the density if pressure increased to 27^{o}C? **(DGK-22)**

**13: **Calculate the mass of 1 dm^{3} of NH_{3} gas at 30°C and 1000 mm Hg pressure, considering that NH_{3} is behaving ideally. **(GJR-19,23)(FSL-19)(DGK-19)(RWP-22)(LHR-22,23)(BWP-22,23)(SRG-23)(SWL-23)**

**14: **Calculate the number of atoms in 20 cm^{3} of CH_{3} gas at 0°C and pressure of 700 mm of Hg. **(RWP-23)**

**15: **State and explain Graham’s law of diffusion. **(RWP-19)**

**3.5: DALTON’S LAW OF PARTIAL PRESSURES**

**16: **State and explain Dalton’s law of partial pressures. Derive its mathematical expression for calculating partial pressure of a gas. **(SWL-17)**

**17: **How Dalton’s law of partial pressures calculates the partial pressure of a gas? **(FSL-21)**

**18: **Derive an equation to find out the partial pressure of a gas knowing the individual moles of the component gases and the total moles of the mixture. **(GJR-21)**

**19: **State Dalton’s law of partial pressures. Also write its mathematical form. Give its one application. **(SWL-17)(FSL-17)(RWP-17)**

**20: **State Dalton’s law of partial pressure and write its four applications. **(LHR-16)**

**21: **Discuss in detail the practical applications of Dalton’s law of partial pressures. **(DGK-21)**

**22: **There is a mixture of hydrogen, helium and methane occupying a vessel of volume 13 dm^{3} at 37°C and pressure of 1 atmosphere. The masses of H_{2} and He are 0.8 g and 0.12 g respectively. Calculate the partial pressure in torr of each gas in the mixture. **(MLT-23)**

**23: **What pressure is exerted by a mixture of 2.00 g of H_{2} and 8.00 g of N_{2} at 273 K in a 10 dm^{3} vessel? **(DGK-23)(FSL-23)(GJR-23)(BWP-23)**

**3.6: DIFFUSION AND EFFUSION**

**24: **What is Graham’s law of diffusion? Give its experimental verification. **(RWP-16)(MLT-16)(FSL-16)(DGK-16,17)(BWP-17)(FSL-17)**

**25: **250 cm^{3} of the sample of hydrogen effuses four times as rapidly as 250 cm^{3} of an unknown gas. Calculate the molar mass of unknown gas. **(SWL-19)(BWP-22)(FSL-22,23)**

**3.7: KINETIC MOLECULAR THEORY OF GASES**

**26: **Give eight postulates of KMT (Kinetic Molecular Theory). **(LHR-16,21)(MLT-17)(GJR-21)**

**27: **Derive Boyle’s and Charles’s laws with the help of kinetic theory of gases. **(MLT-21)**

**28: **Explain Boyle’s law and Avogadro’s law on the basis of KMT. **(MLT-17)**

**29: **What is kinetic interpretation of temperature? Explain. **(DGK-21)**

**3.9: LIQUEFACTION OF GASES**

**30: **What is Joule-Thomson effect? Explain Linde’s method for the liquefaction of gases.** (AJK-16,17)**

**31: **Describe Linde’s method for the liquefaction of gases. **(SRG-17)(RWP-17)**

**3.10: NON-IDEAL BEHAVIOUR OF GASES**

**32: **Explain non-ideal behaviour of gases.** (MLT-16)(BWP-17)**

**3.11: VAN DER WAALS EQUATION FOR REAL GASES**

**33: **Derive van der Waals equation for real gases and give the physical significance for van der Waals’ constants ‘a’ & ‘b’.

**34: **A sample of krypton with a volume of 6.25 dm^{3}, a pressure of 765 torr and a temperature of 20°C is expanded to a volume of 9.55 dm^{3}, and a pressure of 375 torr. What will be the final temperature in ^{o}C? **(SWL-23)**

**35: **One mole of methane gas is maintained at 300 K. Its volume is 250 cm^{3}. Calculate the pressure exerted by the gas under the following conditions: i) When the gas is ideal. ii) When the gas is non-ideal. (a 2.253 atm dm^{6} mol^{–2} b 0.0428 dm^{3} mol^{–1}) **(DGK-19)(LHR-19)(MLT-19,19)(SRG-19)**

**3.12: PLASMA**

**36: **Define plasma and explain its four applications. **(RWP-21)**

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