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10.3.2: Practice Equilibrium Constant Expressions

  • Page ID
    236059
  • Exercise \(\PageIndex{1}\)

    Which of the following is true at equilibrium conditions?  (Choose all that apply.)

    a.  The forward reaction rate is zero.

    b.  The amount of reactants left is zero.

    c.  The forward reaction rate is equal to the reverse reaction rate.

    d.  The amount of products is equal to the amount of reactants.

    e.  The amount of products that is present is constant.

    f.  The product stops forming.

    Answer

    c, e.

    Exercise \(\PageIndex{1}\)

    What does it mean if a reversible reaction has an equilibiurm constant (Keq) with a very small value?

    a.  The reaction rate is very slow.

    b.  There are more reactants than products at equilibrium.

    c.  There are more products than reactants at equilibrium. 

    d.  The forward reaction is slower than the reverse reaction.

    Answer

    b

    Exercise \(\PageIndex{1}\)

    Which of the following would be defined as having a value of 1 in an equilibrium constant expression?  (Choose all that apply.)

    a.  a solid

    b.  a gas

    c.  a liquid

    d.  a solute dissolved in a solution

    Answer

    a and c.

    Exercise \(\PageIndex{1}\)

    \[2 SO_{2 (g)} + O_{2 (g)} \longleftrightarrow 2 SO_{3 (g)}\]

    What is the equilibrium constant expression of the reaction above?

    Answer

    \(K_{eq} = \dfrac{[SO_{3}]^{2}}{[SO_{2}]^{2}[O_{2}]}\)

     

     

     

     

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