Worksheet on Equilibrium Chapter 18

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 1)      Explain the following statements with a sentence

 a)      The concentrations of reactants and products in a system at dynamic equilibrium don’t change.

b)      A change in the pressure on a gaseous system can cause a shift in the equilibrium position.

c)      When a chemical equilibrium is established, the amount of reactants and products is the same.

d)      The Keq for a certain reaction was 2 x 10-7.  This reaction is said to be reactant favored.

e)      When a common ion is added to a system at equilibrium the system shifts to …. 

2)      Calculate Keq for this reaction:  2SO3(g)  à  2SO2(g)  +  O2(g), if the equilibrium concentrations are:  [SO2] = 0.42 M, [O2] = 0.21 M, [SO3] = 0.072 M.

3)      At 25oC, the following reaction has an equilibrium constant of 9.0 x 10-4.  Find the concentration of A(g) in moles per liter, when the concentration of B(g) is 0.030 mol/L and the concentration of C(g) is 0.060 mol/L.

A(g)  ßà  B(g)  +  2C(g)

4)      Indicate how the equilibrium position of this reaction is shifted by the following changes:                   
                      heat +  4HCl(g)  +  O2(g)  ßà  2Cl2(g)  +  2H2O(g)

a)      add Cl2

b)      remove O2

c)      increase pressure

d)      lower the temperature

For each of the changes above state whether the value of Keq would change or not.

Explain one of the adjustments in the equilibrium position above in terms of Le Chatelier’s Principle.

 

5)      At a certain temperature, an equilibrium is established for this reaction in a 3.0 L container:   Cl2(g)  +  Br2(g)  ßà  2BrCl(g).  Given 0.85 mol Cl2, 0.85 mol Br2, and 0.30 mol BrCl, what is Keq?

6)      Aluminum hydroxide has a Ksp of 3.0 x 10-34.  Calculate the equilibrium concentrations of aluminum and hydroxide ions.

7)      Explain what happens when HCl is added to a saturated solution of AgCl?

8)      The solubility of SrCrO4 in water is 1.2 grams per liter of solution.  Calculate Ksp.

 

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