'Equilibrium concentrations' diaporamas de présentation

CHEMICAL EQUILIBRIUM Chapter 16

CHEMICAL EQUILIBRIUM Chapter 16. ALL BOLD NUMBERED PROBLEMS. Properties of an Equilibrium. Equilibrium systems are DYNAMIC (in constant motion) & REVERSIBLE. Cool. Heat. Blue to pink CoCl 4 2- (aq) + 6 H 2 O (l) ? Co(H 2 O) 6 2+ (aq) . Cool. Pink to blue

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Chapter 12 Chemical Equilibrium

Chapter 12 Chemical Equilibrium. The Concept of Equilibrium. Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. The Concept of Equilibrium. Consider colorless frozen N 2 O 4 . At room temperature, it decomposes to brown NO 2 :

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Equilibrium

Equilibrium. Reactions are reversible. A + B C + D ( forward) C + D A + B (reverse) Initially there is only A and B so only the forward reaction is possible As C and D build up, the reverse reaction speeds up while the forward reaction slows down. Eventually the rates are equal.

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Chapter 16 Acids and Bases

Chemistry, The Central Science , 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Chapter 16 Acids and Bases. John D. Bookstaver St. Charles Community College St. Peters, MO ? 2006, Prentice Hall, Inc. Some Definitions. Arrhenius

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Spontaneity and Equilibrium

Spontaneity and Equilibrium. isolated system : . Isothermal process. Maximum work obtained in a process at constant temperature is equal to the decrease in Helmholtz energy of the system. Calculate the maximum work that can be obtained from the combustion of 1 mole of methane at 298 K.

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Weak Acid Titration Calculations

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Unit 4: Equilibrium

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Chemical Equilibrium

Chemical Equilibrium. Chapter 15 AP CHEMISTRY. http://206.180.99.10/~robertsj/AP%20Chapter%20Notes/ap%20ch13.ppt. Chemical Equilibrium. The state where the concentrations of all reactants and products remain constant with time.

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Reaction Rates and Equilibrium

Reaction Rates and Equilibrium. Chapter 17. Collision Theory or Model. Molecules react by colliding with each other with enough energy and proper orientation to break bonds, rearrange and form new bonds

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Unit 4: Equilibrium

Unit 4: Equilibrium. 7.5 Quantitative Changes in Equilibrium Systems. k f. k r. A + 2B AB 2. [AB 2 ]. =. K c =. k f. [A][B] 2. k r. Chemical Kinetics and Chemical Equilibrium. rate f = k f [A][B] 2. rate r = k r [AB 2 ]. Equilibrium rate f = rate r.

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Chemical Equilibrium

Chemical Equilibrium. Basic Skills: Students should be able: To explain the dynamic nature of equilibrium. To be able to write the equilibrium constant expression for a given equilibrium. To explain the connection between an equilibrium and the rates of the forward and reverse reaction.

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Chapter 13: Chemical Equilibrium

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Sections 15.3 Using Equilibrium Constants in Calculations

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Solving Equilibrium problems using the RICE method

Solving Equilibrium problems using the RICE method. General Method. Write the balanced equation for the reaction. Write the equilibrium expression using the law of mass action. List the initial concentrations. Calculate Q to determine the shift to equilibrium.

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ICE Tables

ICE Tables. I nitial (Concentrations) C hange E quilibrium (Concentrations).

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Reaction Reversibility

Reaction Reversibility. ?. 2. 1. Sample problem (similar to 11 & 12). N 2 O 4 ? 2NO 2 . N 2 O 4 : Start = 1.0, finish = 0.20. NO 2 (1.60). Concentration (mol/L). N 2 O 4 (0.20). Time. N 2 O 4 : first find start and finish, then draw curve Start = 1.0, finish = 0.20.

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Equilibrium Law

Equilibrium Law. Mass action expression. Equilibrium constant. Kc =. Introduction to the Equilibrium law. [H 2 O]. [H 2 O] 2. [H 2 ] 2 [O 2 ]. [H 2 ] 2 [O 2 ]. Read 14.3 to PE1. 2H 2 (g) + O 2 (g) ? 2 H 2 O (g). 2 H 2 (g) + O 2 (g) ? 2H 2 O (g). 2H 2 (g) + O 2 (g) ? 2H 2 O (g).

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Equilibrium

Equilibrium. Equilibrium is a macroscopic event, regardless of the direction of approach the forward rate and the reverse rate are the same and changes in concentration cannot be observed. Products favored 10 3 > K > 10 -3 Reactants favored. Heterogeneous Solutions

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Chapter 17: Additional Aspects of Aqueous Equilibria

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