EQUILIBRIUM Equilibrium Constant K Values The equilibrium constant
EQUILIBRIUM
Equilibrium Constant (K Values) The equilibrium constant (Keq) is a number showing the relationship between the concentration of the products and the reactants. Each raised to the power of its coefficient in a balanced equation. True for reversible reactions (go both forwards and backwards).
![Equilibrium Constant Equation � Keq = [Products]coefficients [Reactants]coefficients § Reactants on the left and](http://slidetodoc.com/presentation_image_h2/4ffc9b96931671a24dcf73ceb9d0c08b/image-3.jpg "Equilibrium Constant Equation � Keq = [Products]coefficients [Reactants]coefficients § Reactants on the left and")
Equilibrium Constant Equation � Keq = [Products]coefficients [Reactants]coefficients § Reactants on the left and products on the right § Concentration (molarity) is represented by putting a [bracket] around a formula. � Only use [GASES (g)] and [AQUEOUS (aq)] compounds in Keq expressions because [SOLIDS (s)] and [LIQUIDS (l)] have no concentrations, so they do not need to be included.
Example 3 H 2(g) + N 2(g) 2 NH 3(g) § Write the equilibrium expression for the reaction above: § Keq = [NH 3]2 [H 2]3 [N 2]1 § § § C 3 H 8(g) + 5 O 2(g) 3 CO 2(g) + 4 H 2 O(l) Write the equilibrium expression for the reaction above: The [H 2 O] is not used because it’s a liquid. Keq = [CO 2]3 [C 3 H 8] [O 2]5
What does the calculated value for Keq tell us? A. Keq = 1 means that AT EQUILIBRIUM the [products] = [reactants] B. Keq > 1 means that AT EQUILIBRIUM the [products] > [reactants] C. Keq < 1 means that AT EQUILIBRIUM the [products] < [reactants]
Example 1 A mixture of plenty of gaseous H 2 O and solid C are placed in a large container and allowed to come to equilibrium according to the following reaction: C (s) + H 2 O (g) CO (g) + H 2 (g) The equilibrium concentrations of the species are as follows: [H 2 O] = 0. 56 M, [CO] = 0. 33 M, and [H 2] = 0. 040 M. What is the value of the equilibrium constant for this reaction? Does this equilibrium constant show that there are more products, more reactants, or equal amounts of the products and reactants? AND, how do you know?
![Answer Keq = [CO] [H 2 O] Keq = [0. 33][0. 040] [0. 56]](http://slidetodoc.com/presentation_image_h2/4ffc9b96931671a24dcf73ceb9d0c08b/image-7.jpg "Answer Keq = [CO] [H 2 O] Keq = [0. 33][0. 040] [0. 56]")
Answer Keq = [CO] [H 2 O] Keq = [0. 33][0. 040] [0. 56] = 0. 024 There are more reactants; the value of Keq is smaller than 1
Example 2 Given: 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) The Keq = 6. 67 Write the equilibrium expression Calculate the equilibrium concentration of [SO 3] when… [SO 2] = 0. 25 M and [O 2] = 0. 20 M
Example 3 2 SO 2 (g) + O 2 (g) 2 SO 3 C (s) + H 2 O (g) CO (g) + H 2 (g) Keq = 6. 67 Keq = 0. 024 Which reaction favors the products most? WHY
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