1 / 7

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
Télécharger la présentation

When do you use this?

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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.

More Related