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When do you use this?

You use Keq to find the concentration of a reversible reaction at equilibrium. You use Q to find the concentration of a reversible reaction at a given time before equilibrium to know in which direction the reaction goes. When do you use this?. What are the definitions?.

marcia-jenkins
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When do you use this?

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  1. You use Keq to find the concentration of a reversible reaction at equilibrium. You use Q to find the concentration of a reversible reaction at a given time before equilibrium to know in which direction the reaction goes. When do you use this?

  2. What are the definitions? • Keq: Law of mass action express the relative concentration of reactants and products at equilibrium in terms of quantity called the equilibrium constant • Q: The reaction Quotient of Keq

  3. Steps/Rules • Keq: 1. Balance the equation 2.Put the products on top and the reactants on the bottom 3.coefficients are exponents 4.only use (g) and (aq) 5. Use the M of reactants and products to find keq. Keq>>1= reaction lies to the right Keq<<1= reaction lies to the left Keq=1 at equilibrium

  4. More Steps and Rules Q: 1. Do all for Keq 2.Use given M at given temperature. 3.Compare with value of Keq. Q<Keq= reaction lies to the right (product side) Q>Keq= reaction lies to the left (reactant side)

  5. A solved EXAMPLE (Keq) 2CO(g) + O2 (g) ↔ 2CO2 (g) Keq = [CO2]^2/ [CO]^2 [O2] (Q) COCL2(g) ↔ CO(g) Cl2(g) and Keq =170. If the concentration of CO and C2 are each 0.15M and the concentration of COCL2 is 1.1 x 10^-3 is the reaction at equilibrium? [CO][Cl2] / [COCl2] = (.15)(.15)/1.1x10^-3 = 20 Q=20

  6. Here's Something to SOLVE >:) Keq: NH4NO3 (s) ↔ N2O(g) + H2O Q: At 448 degrees C K= 50.5 for the reaction H2(g) + I2(g) ↔ 2HI (g), Find Q and the direction of the reaction of the reaction if [H2] = .15 M, [I2] = .175 M, [HI] = .950 M.

  7. Here are the answers @_@ • Keq = [N2O][H20]^2 • Q= 34.4. Reaction lies to the right.

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