UNT CHEM 1415 - Chemical Equilibrium Concentration (2 pages)

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Chemical Equilibrium Concentration



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Chemical Equilibrium Concentration

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Concepts describing chemical equilibrium reactions and whether they are homogeneous and heterogeneous


Lecture number:
16
Pages:
2
Type:
Lecture Note
School:
University of North Texas
Course:
Chem 1415 - Gen Chem Engineers
Edition:
1

Unformatted text preview:

CHEM 1415 1st Edition Lecture 16 Unit Chemical Equilibrium Concentration Outline of Current Lecture I Chemical Equilibrium II The Equilibrium Expression III Equilibrium Concentrations a Example 1 Current Lecture Chemical Equilibrium o Dynamic Equilibrium Rates of evaporation or condensation become equal and do not stop at equilibrium and do not go to zero Individual molecules continue to move from the liquid to the vapor phase and back again o The rate of the forward reaction equals the rate of the reverse reaction o Arrows indicate emphasize the dynamic character of the process R P o Reverse reaction Raterev k rev P o Two rates equal at equilibrium Rate for Raterev P k for P eq o k for R k rev k rev R eq The Equilibrium Expression o Using a general chemical reaction aA bB cC dD C c D d o The ratio of concentration is Q a b A B o The expression for the equilibrium constant is always based directly on the reaction stoichiometry o Homogeneous equilibria reactants and products are in the same phase either gaseous or aqueous o Heterogeneous equilibrium multiphase system Equilibrium Concentrations o Strategies to solve equilibrium concentration problems Write a balanced chemical equation for the relevant equilibrium or equilibria These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute Write the corresponding equilibrium expression Create a table of concentrations for all of the reacting species o Example 1 Hydrogen reacts with Iodine gas at elevated temperatures k 59 3 T 400 0 050 M of hydrogen and 0 050 M of Iodine What are the equilibrium concentrations H 2 g I 2 g 2 H I g HI 2 K 59 3 H 2 I 2 H2 I2 HI Initial Concentration 0 050 M 0 050 M 0M Change in Concentration x x 2x Final Concentration 0 050 x 0 050 x 2x HI 2 2 x 2 59 3 K 59 3 2 0 050 x H 2 I 2 2x 7 70 0 050 x 9 70 x 0 39 X 0 040 Therefore H 2 I 2 0 050 0 040 0 010 M HI 2 x 0 080 M



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