Quiz  /  Equilibrium State Class 10 MCQ Questions With Answers

  • 1. 
    At equilibrium

  • All chemical processes have stopped.
  • The [Reactants] = [Products]
  • The concentration of the reactants and products are constant and no longer change.
  • The energy levels of the reactants and products are the same.

  • 2. 
    Select the equilibrium constant for the most reactant favored system.

  • 3.0×10−33.0\times10^{-3}3.0×10−3
  • 7.0×10−37.0\times10^{-3}7.0×10−3
  • 2.0×10−52.0\times10^{-5}2.0×10−5
  • 6.0×10−56.0\times10^{-5}6.0×10−5

  • 3. 
    Which of these will change the value of the equilibrium constant?

  • Increasing the initial amount of one of the reactants.
  • increasing the pressure for a gas phase reaction.
  • increasing the temperature of the system.
  • All of these will change the equilibrium constant.

  • 4. 
    Decreasing the temperature of an endothermic reaction will cause

  • equilibria to shift left and K increases
  • equilibria to shift left and K decreases
  • equilibria to shift right and K increases
  • equilibria to shift right and K decreases

  • 5. 
    2 SO2(g) + O2(g) ⇌ 2 SO3(g)Adding SO3(g) will

  • shift equilibrium right
  • shift equilibrium left
  • increase K
  • have no change

  • 6. 
    For the reaction...N2 (g) + 3 H2(g) ⇌ 2 NH3 (g)If the pressure in the system is increased, which substance(s) will increase in concentration?

  • N2
  • H2
  • N2 and H2
  • NH3

  • 7. 
    What is the equilibrium expression for: Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g)Kc =

  • [Fe]3 [H2O]4 / [Fe3O4] [H2]4
  • [Fe3O4] [H2]4 / [Fe]3 [H2O]4
  • [H2O]4 / [H2]4
  • [Fe] [H2O] / [Fe3O4] [H2]

  • 8. 
    Which of the following is NOT true at equilibrium?

  • The forward and reverse reactions proceed at the same rate.
  • The concentrations of reactants and products do not change.
  • The concentration of the reactants is equal to the concentration of the products.
  • The forward and reverse reactions continue to occur.

  • 9. 
    Which of the following is false about an equilibrium system.

  • The rate of the forward reaction equals the rate of the reverse.
  • Interconversions between reactants and products continue to occur.
  • KcK_cKc​  does not depend on the concentration of reactants and products
  • Raising the temperature always causes the equilibria to shift right.

  • 10. 
    H2(g) + Cl2(g) ⇌ 2 HCl(g)The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

  • equilibrium shifts right
  • equilibrium shifts left
  • You cannot predict the effect
  • no change

  • 11. 
    When Q is greater than KcK_cKc​

  • the [Reactants] will increase and [Products] will decrease
  • the [Reactants] will decrease and [Products] will increase
  • the [Reactants] and [Products] will both increase
  • the [Reactants] and [Products] will both decrease

  • 12. 
    2 SO2(g) + O2(g) ⇌ 2 SO3(g)Removing O2(g) will

  • shift equilibrium right
  • shift equilibrium left
  • increase pressure
  • have no change

  • 13. 
    H2(g)+Cl2(g)⇌2HCl(g)Increasing the pressure will

  • shift equilibrium right
  • shift equilibrium left
  • You cannot predict the effect
  • have no change

  • 14. 
    For the reaction...SO2 + O2 ⇌ SO3If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

  • left
  • right
  • left and right
  • neither left nor right

  • 15. 
    What is the effect of increasing the pressure on the following equilibrium: 2NO(g) + O2 (g) ⇌2NO2(g)?

  • The yield of NO2 increases
  • The yield of NO2 decreases
  • The reaction is slower
  • The concentration of O2 increases.

  • 16. 
    H2(g)+Cl2(g)⇌2HCl(g)The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

  • equilibrium shifts right
  • equilibrium shifts left
  • You cannot predict the effect
  • no change

  • 17. 
    2SO2(g)+O2(g)⇌2SO3(g)Removing O2(g) will

  • shift equilibrium right
  • shift equilibrium left
  • increase pressure
  • have no change

  • 18. 
    What are the two factors to look for when determining if the reaction is at equilibrium?

  • Forward reaction rate is faster than the reverse and concentrations are equal
  • Forward and reverse reaction rates are equal and concentration is constant
  • Forward and revers reaction rates are equal and concentration is equal
  • Forward reaction rate is faster than the reverse and concentration is equal

  • 19. 
    When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in

  • Chemical Equilibrium
  • Chemical Balance
  • Stoichiometry
  • Chemical Reaction

  • 20. 
    2SO2(g)+O2(g)⇌2SO3(g)Adding SO3(g) will

  • shift equilibrium right
  • shift equilibrium left
  • increase K
  • have no change

  • 21. 
    H2(g)+Cl2(g)⇌2HCl(g)Removing Cl2(g) will

  • shift equilibrium right
  • shift equilibrium left
  • increase pressure
  • have no change
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