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Chemistry 1302A/B Study Guide - Final Guide: Equilibrium Constant, Reaction Rate, Supersaturation

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chocolatesheep667

17 Oct 2018

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Western University

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Chemistry 1302A/B

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Document Summary

The cause of k can be very large or very small. If k is large, there are more products than reactions present at equilibrium, lies to the right. If k is small, there are more reactants than products reactions present at equilibrium, lies to the left. Kp is the equilibrium constant where the amounts of the species involved (gases) are measured as pressure (must be atm for fugacity) Kc is the equilibrium constant where the amounts of the species involved (solutions) are measured in molarity (must be m for activity) Only units of m and atm should be used in calculation of kc and kp. The reaction quotient q can be calculated if the amounts of products and reactants can be determined, this number indicates whether the system is at equilibrium. If q = keq, then the system is at equilibrium. If q < keq, then reaction must proceed in forward direction for equilibrium to be attained.

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Related Questions

ENT ives To determine equilibrium concentrations for species in solution . Examine temperature effects on reaction equilibrium Investigate the shift in equilibrium from different stresses on a system kills . Use colorimeter to determine unknown solution concentrations ced .Preparing temperature baths to change reaction conditions tionEquilibrium is defined as a state in which the concentrations of both the reactants and products have no tendency to change with time. We can restate this by saying that the rate of the forward reaction is equal to the rate of the reverse reaction. Recall that with rate we are simply defining how fast a reaction is proceeding, a speed at which the reaction proceeds. Take note that when writing an equilibrium expression, pure liquids (denoted by l or 2) and pure solids (denoted by s) are omitted. Typically we express the equilibrium by K or Kp where c and p denote either concentration or partial pressure respectively. We refer to this value of K, or Kp as an equilibrium constant For any reaction, Kc can be written as the product of the concentration of products, raised to their stoichiometric coefficients, divided by the product of the concentration of the reactants raised to their stoichiometric coefficients. See Equation (5-1) below for an example: aA(aq) + bB(aq-cC(aq) + dD(aq) (5-1) A] [B]b As mentioned before, K, or K, are equilibrium constants meaning that they will have the same value unless temperature is changed. This brings in two important ideas 1) We can perturb the equilibrium concentrations of a reaction, say [A] for instance which will cause the other concentrations to shift so that K for the reaction remains constant. 2) If we change temperature, we will either increase or decrease our value of K depending on the specific reaction we are examining. Determining K, and Equilibrium Concentrations During lecture we often discuss the idea of using ICE tables as a method for organizing and calculating concentrations of reactions as they proceed towards equilibrium. In a typical ICE table you need to know initial concentrations and the magnitude of K to determine the equilibrium concentrations. Alternatively, if you know the equilibrium concentrations for a reaction you can calculate K. For this experiment we will be examining a complex ion formation, when iron(III) ion