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CHEM 120 Lecture Notes - Lecture 18: Reaction Mechanism, Joule, Inert Gas

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15 Apr 2016

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CHEM 120 Full Course Notes

CHEM 120 Full Course Notes

Document Summary

The signiicance of the magnitude of the equilibrium constant. The equilibrium condiion is achieved, in general, for a condiion where the system has a non-zero concentraion of both reactant and product species. The most important tool we have for handling reacions at equilibrium is the equilibrium constant. Really iny kp = mostly reactants / reactants are strongly favored. Signiicant quaniies of both reactants and products are likely to be present at equilibrium only if ~10-10 < k < ~1010. The equilibrium constant determines those concentraions: reacions under kineic control: concentraion of products and reactants depends on the rates of reacion (ie. k & ea). Earlier, before reaching equilibrium, the reacions are under kineic control, but once reaching equilibrium, they become under thermodynamic control. Diamonds do not turn into graphite because of the enormous acivaion energy barrier. The reacion quoient (q) is used in predicing the direcion of net change. [ a ]t g [ h ]t a[ b]t.

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Related Questions

The equilibrium constant for HI decomposition at 500 Â°C is5.8Ã10-3.

2HI(g) <=> H2(g) + I2(g)

At that temperature reactants and products are gaseous. (There isno change in the total number of moles, so Kc = Kp.)
A sample of 0.40 mol of HI is placed in a 1.00 L vessel which isthen heated to 500 Â°C. When equilibrium is reached, what is themolar concentration of H2? (Give units).

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