CHEM 135 1st Edition Lecture 15 Outline of Last Lecture I Practice Problems II Read section 13 7 and watch video posted on BB Outline of Current 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 Current Lecture Chemical Equilibrium N2 3H2 2NH3 This equation can go both ways and is reversible The rates of the reaction are the same meaning they are at equilibrium no significant change in concentration Does this mean the reaction stops No there is constant movement even in equilibrium in order to keep the reaction balanced Reversible Reactions and Equilibrium Constants aA bB cC dD 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 Rates of the forward and reverse reactions are equal at equilibrium Equilibrium does NOT mean the products are equal K eq products reactants K eq C c D d A a B b The constant within this equation is unitless Ex CH4 4Cl2 CCl4 4HCl CCl HCl 4 4 K eq Ex C3H8 5O2 3CO2 4H2O O H2 4 O2 5 CO2 3 K eq If Keq 1 it consists of more product than reactant greater numerator If Keq 1 it consist of more reactant than product greater denominator Heterogeneous Equilibrium Reactants and products are in different phases o 2CO2 g CO2 g C s CO C O2 2 o Equilibrium constant 2 KC Do not include pure solids and pure liquids in an equilibrium constant Changing the amount of solid does not change the concentration of gas Ex Solve the following expressions and determine whether or not it favors the products or reactants 1 SnO2 s 2CO g Sn s 2CO2 g CO2 2M CO 2M CO 2 2 K eq This equation favors neither the reactant nor product 2 NaCl s H2SO4 l HCl g NaHSO4 s HCl 3M K eq HCl 3 This equation favors the product 3 P4 s 6NO g P4O6 s 3N2 g N 2 3 NO 6 K eq This reaction favors the reactant NO 2M N2 2
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