1 / 14

INTRODUCTION TO EQUILIBRIUM

INTRODUCTION TO EQUILIBRIUM. Kinetics Explains how chemical reactions take place and some of the factors that affect the reactions’ speed Equilibrium when the rate of opposing forces are equal Remember equilibrium with respect to vapor pressure or dissolving.

nora
Télécharger la présentation

INTRODUCTION TO EQUILIBRIUM

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. INTRODUCTION TO EQUILIBRIUM

  2. Kinetics • Explains how chemical reactions take place and some of the factors that affect the reactions’ speed • Equilibrium • when the rate of opposing forces are equal • Remember equilibrium with respect to vapor pressure or dissolving

  3. A few chemical reactions go to completion • Using up one or more reactants and then stopping • Many reactions behave a different way… • aA + bB cC + dD • At first A and B start to form C and D • But then, C and D start to react to form A and B • cC + dD  aA + bB • These two reactions proceed until the two rats of reaction become equal • CHEMICAL EQUILIBRIUM has been reached

  4. Chemical equilibrium • Is reached when the rate of the forward reaction is equal to the rate of the reverse reaction • The reaction does not stop • The rates are the same but the forward and reverse reactions are still happening • Because the rates are the same, the net change in the concentration of A, B, C and D become constant. • DYNAMIC EQUILIBRIUM • Aa + bB↔ cC + dD

  5. It is important to remember that at equilibrium the concentrations of chemical species are constant, but not necessarily equal.

  6. Law of mass action • General description of equilibrium condition

  7. jA + kB --> nC + mD K = [C]n[D]m[A]j[B]k • [A] indicates conc@ equilibrium!! • K= equilibrium constant

  8. Haber process • Write law of mass action for forward rxn • [NH3] = 3.1 x 10-2mol/L • [N2] = 8.5 x 10-1mol/L • [H2] = 3.1 x 10-3mol/L

  9. Now calculate • Value of K • value of K of reverse rxn • K for the following rxn • 1/2N2(g) + 3/2H2(g) --> NH3(g)

  10. Some important info • If rxn reversed • K’ = 1/K • Original factor multipled • K’’ = Kn (# that is mult)

  11. UNITS! • Depends on powers of various conc in law of mass action

  12. Applications • K values are always the same at specific temps regardless of the amts of reactants that are mixed together initially

  13. Ratio defined • Although K is always the same, the equilibrium conc will not always be the same

More Related