Equilibrium Calculations Comparing K to Q. Value of the Equilibrium Constant K tells where the equilibrium lies How likely (to what extent) the reaction.

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Presentation transcript:

Equilibrium Calculations Comparing K to Q

Value of the Equilibrium Constant K tells where the equilibrium lies How likely (to what extent) the reaction is to occur Does not give rate (that’s KINETICS) Three possibilities  K = 1 Equal ratio of products to reactants Equilibrium lies in the “middle”

Value of the Equilibrium Constant K tells where the equilibrium lies How likely (to what extent) the reaction is to occur Does not give rate (that’s KINETICS) Three possibilities  K >1 Bigger number on top, so… More products Equilibrium favors the PRODUCTS (to the right)

Value of the Equilibrium Constant K tells where the equilibrium lies How likely (to what extent) the reaction is to occur Does not give rate (that’s KINETICS) Three possibilities  K <1 Bigger number on bottom, so… More reactants Equilibrium favors the REACTANTS (to the left)

Practice Problem #1 H 2(g) + Cl 2(g)  HCl (g) At equilibrium [H 2 ] = 0.42 M, [Cl 2 ] = M, and [HCl] = 0.95 M. Determine the equilibrium constant.

Practice Problem #2 C (s) + CO 2(g)  CO (g) K c = 6.5 At equilibrium some CO 2, 5.4×10 -5 moles of CO, and 1.88 x moles of C exist in a L container. How many moles of CO 2 exist at equilibrium?

Practice Problem #3 CO 2(g) + H 2(g)  CO (g) + H 2 O (g) Calculate the value of the equilibrium constant, K c, for the system shown, if moles of CO 2, moles of H 2, moles of CO, and moles of H 2 O vapor were present in a 2.00 L reaction vessel were present at equilibrium.

Practice Problem #4 N 2 O 4 (g)  2 NO 2 (g) A sample of N 2 O 4 (g) is allowed to come to equilibrium with NO 2 (g) in a 750 mL flask. At equilibrium, 38.6 g N 2 O 4 remains and moles of NO 2 have been produced. Calculate the equilibrium constant, Kc, for the reaction.

Reaction Quotient (Q) Where you are at

Reaction Quotient (Q) Snapshot of reaction at some point Same calculation as K c They will give you the K of the reaction Compare Q and K = [C] c [D] d [A] a [B] b

Reaction Quotient (Q) Example: 2 NO 2 (g)  N 2 O 4 (g) K p = 100°C AT SOME POINT, moles of NO 2 are mixed with moles of N 2 O 4 in a 4.00 L flask at 100°C. = [P N 2 O 4 ] [P NO 2 ] 2 = 0.654

Reaction Quotient (Q) Where am I?? K p = 11, Q = Compare Q to K to see where you are 3 situations  Q = K At EQUILIBRIUM!!

Reaction Quotient (Q) Where am I?? K p = 11, Q = Compare Q to K to see where you are 3 situations  Q > K Bigger number, so… Favors products Must shift left (towards reactants to get to equilibrium)

Reaction Quotient (Q) Where am I?? K p = 11, Q = Compare Q to K to see where you are 3 situations  Q < K Smaller number, so… Favors reactants Must shift right (towards products to get to equilibrium)