First set of notes following Exam 2
First set of notes following Exam 2 chem 10061-001
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This 2 page Class Notes was uploaded by Matthew Goetz on Wednesday March 30, 2016. The Class Notes belongs to chem 10061-001 at Kent State University taught by David bowers in Summer 2015. Since its upload, it has received 24 views. For similar materials see general chemistry 2 in Chemistry at Kent State University.
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Date Created: 03/30/16
Gen Chem 2 Notes Following Exam 2 Chapter 17 will focus on the extent of a reaction. To put this in simpler terms, we will examine at what point in time a reaction reaches equilibrium! Therefore, we won’t be calculating speed of reactions, just at what point do they reach equilibrium (if they ever do in the particular reaction we are examining), and how much product has formed once equilibrium is reached. At equilibrium, no net change will occur in the reaction’s concentrations. Kc is equal to the concentrations of gaseous products divided by concentrations of gaseous reactants. (This is the easiest way for me to express the equation that we use). If K is very small then the reaction yields little product before reaching equilibrium. This is described as the reaction favors reactants. If K is very large then it is the opposite. Reaction Quotient (Q) Ratio of products to reactants. This is calculated the same as K. However, they are different because Q may be calculated at any point in a reaction and K may only be calculated at equilibrium! At equilibrium though, Q = K. If this isn’t true then the reaction must continue. If Q is smaller than K then the reaction must continue towards products. If Q is larger than K then the reaction must continue towards reactants. Once again, in these calculations we need not consider solids nor pure liquids because their concentrations don’t change. Kp is very similar to Kc, thought Kp deals with the partial pressures of the gases that are present while Kc deals with the concentrations of them. They are calculated in the same manner though. A modified version of the ideal gas law allows us to change between Kc and Kp: Kp = Kc (RT)^Δn R is a given constant, .0821 T is the temperature in Kelvin And n is the moles of product minus the moles of reactants. If you are trying to solve for K or Q but you are missing more than one variable you must construct an ICE table! An example of an ICE table is given here: In this example, to solve for x you would make the top of the problem x^2, and then bottom of the problem would be (.100x) ^2). Since this is a perfect square you could merely take the square root of the entire problem and then solve for x from there. Once you have x you would plug it into the equilibrium part of the ICE table told solve for the concentrations of each product and reactant at equilibrium.
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