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BU CHEM 108 - Chemical Equilibrium Review
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Chem 108 1st Edition Lecture 17Current LectureChapter 15: Chemical equilibrium reviewedEquilibrium constant: - Equilibrium Constant Expression: Ratio of equilibrium concentrations or partial pressures of products to reactants, each term raised to a power equal to the coefficient of that substance in the balanced chemical equation.- K = ([C]c[D]d)/([A]a[B]b) = (Products/reactants)o where [A], [B], etc., are equilibrium concentrationso where [A], [B], etc., could also be partial pressure- K>>1 equilibrium lies to the right: the concentration of the products is greater than the concentration of the reactants - K<<1 equilibrium lies to the left: the concentration of the reactants is greater than the concentration of the products- K=0 no reaction- K = infinite, irreversible reactionEquilibrium in the Gas Phase:- Kp = Kc (RT)Δno Δn = number of moles of gaseous products minus the number of moles of gaseous reactantso Kp = equilibrium constant using partial pressure o Kc = equilibrium constant using concentration - Kp = Kc /(RT) (an equation without moles)Types of Equilibrium: - Amount of pure solid and pure liquid product or reactants do not affect the equilibrium in a heterogeneous reaction. This is because any pure solid and pure liquid have constant concentrations because their mass and number of moles per unit of volume are always the same.o Homogeneous equilibrium: Equilibrium involving reactants and products in the same phase.o Heterogeneous equilibrium: Equilibrium involving reactants and products in more than one phaseLe Châtelier’s Principle- Factors that will change the relative rates of forward/reverse reactions, or change the value of Q compared to K, will cause a shift in the position of equilibrium.- If you add or take away products or reactants, the reaction would shift until equilibrium was reachedEffects of Temperature and pressure on equilibrium:- The value of K for an endothermic reaction increases with increasing temperature, and the valueof K for an exothermic reaction decreases with increasing temperature. - Equilibrium shifts in response to an increase or decrease in volume caused by a decrease or increase in pressure toward the side with fewer moles of gases.Calculating concentrations/ partial pressures of reactants and products:- Use the I.C.E table to develop algebraic terms for each reactants and products concentration/partial pressure at equilibrium. Let x be the change in concentration/partial pressure of each component of the reaction. Express the changes in terms of x and substitute these terms into the expression for K and solve for x. Quadratic


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BU CHEM 108 - Chemical Equilibrium Review

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