Chemistry · Textbook solutions

Chemical Equilibrium

Every solved example, exercise, and miscellaneous question — in the order the textbook teaches them. · 25 questions

12. Chemical Equilibrium — worked examples

6 q

Solved Examples

Worked · 6
  1. Solved Ex.12.1
    Write the rate equation for the following reaction: i. C+O2⟶CO2\mathrm{C} + \mathrm{O_2} \longrightarrow \mathrm{CO_2} ii. 2KClO3⟶2KCl+3O22\mathrm{KClO_3} \longrightarrow 2\mathrm{KCl} + 3\mathrm{O_2}
  2. Solved Ex.12.2
    N2(g)+3H2(g)⇌2NH3(g)\mathrm{N_2(g)} + 3\mathrm{H_2(g)} \rightleftharpoons 2\mathrm{NH_3(g)} Write expression for KPK_P in terms of KcK_c.
  3. Solved Ex.12.3
    Write an expression for KPK_P and relate it to KcK_c for the following reversible reaction. H2(g)+I2(g)⇌2HI(g)\mathrm{H_2(g)} + \mathrm{I_2(g)} \rightleftharpoons 2\mathrm{HI(g)}
  4. Solved Ex.12.4
    Write the equilibrium constant expression for the decomposition of baking soda. Deduce the unit of KCK_C from the above expression.
  5. Solved Ex.12.5
    Equal concentrations of hydrogen and iodine are mixed together in a closed container at 700 K and allowed to come to equilibrium. If the concentraion of HI at equilibrium is 0.85 mol dm−30.85\ \mathrm{mol\ dm^{-3}}, what are the equilibrium concentrations of H2\mathrm{H_2} and I2\mathrm{I_2} if KC=54K_C = 54 at this temperature ?
  6. Solved Ex.12.6
    The equilibrium constant KCK_C for the reaction of hydrogen with iodine is 54.0 at 700 K. H2(g)+I2(g)⇌2HI(g)\mathrm{H_2(g)} + \mathrm{I_2(g)} \rightleftharpoons 2\mathrm{HI(g)} KC=54.0K_C = 54.0 at 700 K a. If kfk_f is the rate constant for the formation of HI and krk_r is the rate constant for the decomposition of HI, deduce whether kfk_f is larger or smaller than krk_r. b. If the value of krk_r at 700 K is 1.16×10−31.16 \times 10^{-3}, what is the kfk_f ?

Exercises

19 q

1. Choose the correct option

Practice · 4
  1. Choose the correct option
    Ex Q.1 (A)
    The equlilibrium , H2O(l)⇌H⊕(aq)+OH(aq)\mathrm{H_2O(l)} \rightleftharpoons \mathrm{H^{\oplus}(aq)} + \mathrm{OH(aq)} is
    1. A.
      dynamic
    2. B.
      static
    3. C.
      physical
    4. D.
      mechanical
  2. Ex Q.1 (B)
    For the equlibrium, A⇌2B+Heat\mathrm{A} \rightleftharpoons 2\mathrm{B} + \text{Heat}, the number of 'A' molecules increases if
    1. A.
      volume is increased
    2. B.
      temperature is increased
    3. C.
      catalyst is added
    4. D.
      concerntration of B is decreased
  3. Ex Q.1 (C)
    For the equilibrium Cl2(g)+2NO(g)⇌2NOCl(g)\mathrm{Cl_2(g)} + 2\mathrm{NO(g)} \rightleftharpoons 2\mathrm{NOCl(g)} the concerntration of NOCl will increase if the equlibrium is disturbed by
    1. A.
      adding Cl2\mathrm{Cl_2}
    2. B.
      removing NO
    3. C.
      adding NOCl
    4. D.
      removal of Cl2\mathrm{Cl_2}
  4. Ex Q.1 (E)
    When volume of the equilibrium reaction C(g)+H2O(g)⇌CO(g)+H2(g)\mathrm{C(g)} + \mathrm{H_2O(g)} \rightleftharpoons \mathrm{CO(g)} + \mathrm{H_2(g)} is increased at constant temperature the equilibrium will
    1. A.
      shift from left to right
    2. B.
      shift from right to left
    3. C.
      be unaltered
    4. D.
      can not be predicted

2. Answer the following

Practice · 10
  1. Answer the following
    Ex Q.2 (A)
    State Law of Mass action.
  2. Ex Q.2 (B)
    Write an expression for equilibrium constant with respect to concerntration.
  3. Ex Q.2 (C)
    Derive mathematically value of kPk_P for for A(g)+B(g)⇌C(g)+D(g)\mathrm{A(g)} + \mathrm{B(g)} \rightleftharpoons \mathrm{C(g)} + \mathrm{D(g)}
  4. Ex Q.2 (D)
    Write expressions of KcK_c for following chemical reactions i. 2SO2(g)+O2(g)⇌2SO3(g)2\mathrm{SO_2(g)} + \mathrm{O_2(g)} \rightleftharpoons 2\mathrm{SO_3(g)} ii. N2O4(g)⇌2NO2(g)\mathrm{N_2O_4(g)} \rightleftharpoons 2\mathrm{NO_2(g)}
  5. Ex Q.2 (E)
    Mention various applications of equilibrium constant.
  6. Ex Q.2 (F)
    How does the change of pressure affect the value of equilibrium constant ?
  7. Ex Q.2 (J)
    Differentiate irreversible and reversible reaction.
  8. Ex Q.2 (K)
    Write suitable conditions of concentration, temperature and pressure used during manufacture of ammonia by Haber process.
  9. Ex Q.2 (L)
    Relate the terms reversible reactions and dynamic equilibrium.
  10. Ex Q.2 (M)
    For the equilibrium. BaSO4(s)⇌Ba2⊕(aq)+SO42⊖(aq)\mathrm{BaSO_4(s)} \rightleftharpoons \mathrm{Ba^{2\oplus}(aq)} + \mathrm{SO_4^{2\ominus}(aq)} state the effect of a. Addition of Ba2⊕\mathrm{Ba^{2\oplus}} ion. b. Removal of SO42⊖\mathrm{SO_4^{2\ominus}} ion c. Addition of BaSO4(s)\mathrm{BaSO_4(s)} on the equilibrium.

3. Explain

Practice · 5
  1. Explain :
    Ex Q.3 (A)
    Dynamic nature of chemical equilibrium with suitable example.
  2. Ex Q.3 (B)
    Relation between KcK_c and KpK_p.
  3. Ex Q.3 (C)
    State and explain Le Chatelier's principle with reference to 1. change in temperature 2. change in concerntration.
  4. Ex Q.3 (D)
    a. Reversible reaction b. Rate of reaction
  5. Ex Q.3 (E)
    What is the effect of adding chloride on the position of the equilibrium ? AgCl(s)⇌Ag⊕(aq)+Cl⊖(aq)\mathrm{AgCl(s)} \rightleftharpoons \mathrm{Ag^{\oplus}(aq)} + \mathrm{Cl^{\ominus}(aq)}