Chemistry · Textbook solutions

States of Matter

Every solved example, exercise, and miscellaneous question — in the order the textbook teaches them. · 50 questions

10. States of Matter — worked examples

8 q

Solved Examples

Worked · 8
  1. Solved Ex.10.1
    The volume occupied by a given mass of a gas at 298 K is 25 mL at 1 atmosphere pressure. Calculate the volume of the gas if pressure is increased to 1.25 atmosphere at constant temperature.
  2. Solved Ex.10.2
    At 300 K a certain mass of a gas ocupies 1×10−4 dm31 \times 10^{-4}\ \mathrm{dm^3} volume. Calculate its volume at 450 K and at the same pressure.
  3. Solved Ex.10.3
    A sample of N2\mathrm{N_2} gas was placed in a flexible 9.0 L container at 300 K at a pressure of 1.5 atm. The gas was compressed to a volume of 3.0 L and heat was added until the temperature reached 600 K. What is the new pressure inside the container?
  4. Solved Ex.10.4
    Find the temperature in ∘C^\circ\mathrm{C} at which volume and pressure of 1 mol of nitrogen gas becomes 10 dm310\ \mathrm{dm^3} and 2.46 atmosphere respectively.
  5. Solved Ex.10.5
    A mixture of 28 g N2\mathrm{N_2}, 8 g He and 40 g Ne has 20 bar pressure. What is the partial pressure of each of these gases ?
  6. Solved Ex.10.5b
    Water has Tc=647.1 K\mathrm{T_c} = 647.1\ \mathrm{K} and Pc=220.6 bar\mathrm{P_c} = 220.6\ \mathrm{bar}. What do these values imply about the state of water under ordinary conditions?
  7. Solved Ex.10.6
    CO2\mathrm{CO_2} has Tc=38.98 ∘C\mathrm{T_c} = 38.98\ ^\circ\mathrm{C} and Pc=73 atm\mathrm{P_c} = 73\ \mathrm{atm}. How many phases of CO2\mathrm{CO_2} coexist at (i) 50 ∘C50\ ^\circ\mathrm{C} and 73 atm, (ii) 20 ∘C20\ ^\circ\mathrm{C} and 50 atm.
  8. Solved Ex.10.7
    In which of the following cases water will have the highest and the lowest boiling point ? Water is boiled a. in an open vessel, b. in a pressure cooker, c. in a evacuated vessel.

Exercise

42 q

1. Select and write the most appropriate alternatives from the given choices

Practice · 5
  1. Select and write the most appropriate alternatives from the given choices.
    Ex Q.1 (A)
    The unit of viscosity is
    1. A.
      dynes
    2. B.
      newton
    3. C.
      gram
    4. D.
      poise
  2. Ex Q.1 (B)
    Which of the following is true for 2 moles of an ideal gas ?
    1. A.
      PV=nRT\mathrm{PV} = n\mathrm{RT}
    2. B.
      PV=RT\mathrm{PV} = \mathrm{RT}
    3. C.
      PV=2RT\mathrm{PV} = 2\mathrm{RT}
    4. D.
      PV=T\mathrm{PV} = \mathrm{T}
  3. Ex Q.1 (C)
    Intermolecular forces in liquid are -
    1. A.
      greater than gases
    2. B.
      less than solids
    3. C.
      both a and b
    4. D.
      greater than solids
  4. Ex Q.1 (D)
    Interactive forces are .......... in ideal gas.
    1. A.
      nil
    2. B.
      small
    3. C.
      large
    4. D.
      same as that of real gases
  5. Ex Q.1 (E)
    At constant temperature the pressure of 22.4 dm322.4\ \mathrm{dm^3} volume of an ideal gas was increased from 105 kPa to 210 kPa, New volume could be-
    1. A.
      44.8 dm344.8\ \mathrm{dm^3}
    2. B.
      11.2 dm311.2\ \mathrm{dm^3}
    3. C.
      22.4 dm322.4\ \mathrm{dm^3}
    4. D.
      5.6 dm35.6\ \mathrm{dm^3}

2. Answer in one sentence

Practice · 10
  1. Answer in one sentence.
    Ex Q.2 (A)
    Name the term used for mixing of different gases by random molecular motion and ferquent collision.
  2. Ex Q.2 (B)
    The pressure that each individual gas would exert if it were alone in the container, what do we call it as ?
  3. Ex Q.2 (C)
    When a gas is heated the particles move more quickly. What is the change in volume of a heated gas if the pressure is kept constant ?
  4. Ex Q.2 (D)
    A bubble of methane gas rises from the bottom of the North sea. What will happen to the size of the bubble as it rises to the surface ?
  5. Ex Q.2 (E)
    Convert the following temperatures from degree celcius to kelvin. a. −15 ∘C-15\ ^\circ\mathrm{C} b. 25 ∘C25\ ^\circ\mathrm{C} c. −197 ∘C-197\ ^\circ\mathrm{C} d. 273 ∘C273\ ^\circ\mathrm{C}
  6. Ex Q.2 (F)
    Convert the following pressure values into Pascals. a. 10 atmosphere b. 1 kPa. c. 107000 Nm−2107000\ \mathrm{Nm^{-2}} d. 1 atmosphere
  7. Ex Q.2 (G)
    Convert : a. Exactly 1.5 atm to pascals b. 89 kPa to newton per square metre (Nm−2)(\mathrm{Nm^{-2}}) c. 101.325 kPa to bar d. −100 ∘C-100\ ^\circ\mathrm{C} to kelvin e. 0.124 torr to standard atmosphere
  8. Ex Q.2 (H)
    If density of a gas is measured at constant temperature and pressure then which of the following statement is correct ?
    1. A.
      Density is directly proportional to molar mass of the gas.
    2. B.
      Greater the density greater is the molar mass of the gas.
    3. C.
      If density, temperature and pressure is given ideal gas equation can be used to find molar mass.
    4. D.
      All the above statements are correct.
  9. Ex Q.2 (I)
    Observe the following conversions. Which of the above reactions is in accordance with the priciple of stoichiometry ?
  10. Ex Q.2 (J)
    Hot air balloons float in air because of the low density of the air inside the balloon. Explain this with the help of an appropriate gas law.

3. Answer the following questions

Practice · 10
  1. Answer the following questions.
    Ex Q.3 (A)
    Identify the gas laws from the following diagrams.
  2. Ex Q.3 (B)
    Consider a sample of a gas in a cylinder with a movable piston. Show digramatically the changes in the position of piston, if - a. Pressure is increased from 1.0 bar to 2.0 bar at constant temperature. b. Temperature is decreased from 300 K to 150 K at constant pressure c. Temperature is decreased from 400 K to 300 K and pressure is decreased from 4 bar to 3 bar.
  3. Ex Q.3 (D)
    List the characteristic physical properties of the gases.
  4. Ex Q.3 (E)
    Define the terms : a. Polarizability b. Hydrogen bond c. Aqueous tension d. Dipole moment
  5. Ex Q.3 (F)
    Would it be easier to drink water with a straw on the top of the Mount Everest or at the base ? Explain.
  6. Ex Q.3 (G)
    Identify type of the intermolecular forces in the following compounds. a. CH3−OH\mathrm{CH_3-OH} b. CH2=CH2\mathrm{CH_2{=}CH_2} c. CHCl3\mathrm{CHCl_3} d. CH2Cl2\mathrm{CH_2Cl_2}
  7. Ex Q.3 (H)
    Name the types of intermolecular forces present in Ar\mathrm{Ar}, Cl2\mathrm{Cl_2}, CCl4\mathrm{CCl_4} and HNO3\mathrm{HNO_3}
  8. Ex Q.3 (I)
    Match the pairs of the following :
    'A''B'
    a. Boyle's lawi. at constant pressure and volume
    b. Charles' lawii. at constant temperature
    iii. at constant pressure
  9. Ex Q.3 (J)
    Write the statement for : (a) Boyle's law (b) Charles' law
  10. Ex Q.3 (K)
    Differentiate between Real gas and Ideal gas.

4. Answer the following questions

Practice · 5
  1. Answer the following questions
    Ex Q.4 (A)
    State and write mathematical expression for Dalton's law of partial pressure and explain it with suitable example.
  2. Ex Q.4 (B)
    Derive an Ideal gas equation. Mention the terms involved in it. Also write how it is utilised to obtain combined gas law.
  3. Ex Q.4 (C)
    With the help of graph answer the following - At constant temperature, a. Graph shows relation between pressure and volume. Represent the relation mathematically. b. Identify the law. c. Write the statement of law.
  4. Ex Q.4 (D)
    Write Postulates of kinetic theory of gases.
  5. Ex Q.4 (E)
    Write a short note on - a. Vapour pressure. b. Surface tension c. Viscosity.

5. Solve the following

Practice · 12
  1. Solve the following (Constants supplied by the chapter, for the items that need them : gas constant R=0.0821 dm3 atm K−1 mol−1=8.314 J K−1 mol−1\mathrm{R} = 0.0821\ \mathrm{dm^3\ atm\ K^{-1}\ mol^{-1}} = 8.314\ \mathrm{J\ K^{-1}\ mol^{-1}} (Table 10.4), Avogadro number NA=6.022×1023 mol−1\mathrm{N_A} = 6.022 \times 10^{23}\ \mathrm{mol^{-1}}.)
    Ex Q.5 (A)
    A balloon is inflated with helium gas at room temperature of 25 ∘C25\ ^\circ\mathrm{C} and at 1 bar pressure when its initial volume is 2.27 L and allowed to rise in air. As it rises in the air external pressure decreases and the volume of the gas increases till finally it bursts when external pressure is 0.3 bar. What is the limit at which volume of the balloon can stay inflated ?
  2. Ex Q.5 (B)
    A syringe has a volume of 10.0 cm310.0\ \mathrm{cm^3} at pressure 1 atm. If you plug the end so that no gas can escape and push the plunger down, what must be the final volume to change the pressure to 3.5 atm?
  3. Ex Q.5 (C)
    The volume of a given mass of a gas at 0 ∘C0\ ^\circ\mathrm{C} is 2 dm32\ \mathrm{dm^3}. Calculate the new volume of the gas at constant pressure when a. The temperature is increased by 10 ∘C10\ ^\circ\mathrm{C}. b. The temperature is decreased by 10 ∘C10\ ^\circ\mathrm{C}.
  4. Ex Q.5 (D)
    A hot air balloon has a volume of 2800 m32800\ \mathrm{m^3} at 99 ∘C99\ ^\circ\mathrm{C}. What is the volume if the air cools to 80 ∘C80\ ^\circ\mathrm{C}?
  5. Ex Q.5 (E)
    At 0 ∘C0\ ^\circ\mathrm{C}, a gas occupies 22.4 liters. How nuch hot must be the gas in celsius and in kelvin to reach volume of 25.0 literes?
  6. Ex Q.5 (F)
    A 20 L container holds 0.650 mol of He gas at 37 ∘C37\ ^\circ\mathrm{C} at a pressure of 628.3 bar. What will be new pressure inside the container if the volume is reduced to 12 L. The temperature is increased to 177 ∘C177\ ^\circ\mathrm{C} and 1.25 mol of additional He gas was added to it?
  7. Ex Q.5 (G)
    Nitrogen gas is filled in a container of volume 2.32 L at 32 ∘C32\ ^\circ\mathrm{C} and 4.7 atm pressure. Calculate the number of moles of the gas.
  8. Ex Q.5 (H)
    At 25 ∘C25\ ^\circ\mathrm{C} and 760 mm of Hg pressure a gas occupies 600 mL volume. What will be its pressure at the height where temperature is 10 ∘C10\ ^\circ\mathrm{C} and volume of the gas 640 mL ?
  9. Ex Q.5 (I)
    A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5 g neon. If pressure of the mixture of the gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture?
  10. Ex Q.5 (J)
    Calculate the pressure in atm of 1.0 mole of helium in a 2.0 dm32.0\ \mathrm{dm^3} container at 20.0 ∘C20.0\ ^\circ\mathrm{C}.
  11. Ex Q.5 (K)
    Calculate the volume of 1 mole of a gas at exactly 20 ∘C20\ ^\circ\mathrm{C} at a pressure of 101.35 kPa.
  12. Ex Q.5 (L)
    Calculate the number of molecules of methane in 0.50 m30.50\ \mathrm{m^3} of the gas at a pressure of 2.0×102 kPa2.0 \times 10^{2}\ \mathrm{kPa} and a temperature of exactly 300 K.