CHEM 135 1st Edition Lecture 16 Outline of Last Lecture I Chemical Equilibrium a Introduction b Definition II Reversible reactions and Equilibrium Constant a Definitions b Equations c Examples III Heterogeneous Equilibrium a Definition b Examples Outline of Current Lecture I Calculating equilibrium constant a Examples b Kc vs Kp II Reaction Quotient a Equation definition b Examples Current Lecture Calculating equilibrium constant from measured concentrations Ex I2 g 2I g Kc 0 011 I2 eq 0 1M I 2 K eq I 2 I 2 2 I K eq I 2 I eq 0 033 M 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 Kc concentration Kp partial pressure The relationship between the two constants is as follows Kp Kc RT n Ex PCl5 decomposes to PCl3 and Cl2 If the initial concentration of PCl5 200M and it s final concentration is 120M what is the equilibrium constant 1 Create an ICE table PCl5 PCl3 Cl2 Initial 0 02 0 0 0 0 Change 0 08 0 08 0 08 Equilibrium 0 12 0 08 0 08 Cl 2 eq PCl PC l 3 eq K eq 0 08 0 08 0 0533 0 12 Reaction Quotient Q K products at equilibrium reactants Q products at any point the reaction reactants The reaction quotient determines which direction the reaction will take place o Q K majority of reactants move to the right to reach eq R P o Q K majority of products move to the left to reach eq P R Ex The equilibrium constant for the reaction is 2A 3B is 2 3 If A 0 10M and B 0 050M which direction will the reaction take place B 3 A 2 Q Q 0 125 Q K the reaction must proceed to the right
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