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CHM136H1 Chapter Notes - Chapter 7: Dynamic Equilibrium, Equilibrium Constant, Reaction Rate

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27 Aug 2016

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C.Scott Browning

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CHM136H1 Full Course Notes

CHM136H1 Full Course Notes

Document Summary

Physical systems evaporation condensation rate of evaporation= rate of condensation (no net change in amount of liquid + gas) > system reached equilibrium only occur in closed system. Concentrations of reactants + products remain constant at equilibrium they are being produced and destroyed at an equal rate. At equilibrium there is no change in macroscopic properties. Equilibrium can be reached from either direction observable properties e. g. color + density. These don"t change as they depend on the concentrations of the components of the mixture. Same equilibrium mixture will result under the same conditions, no matter whether the reaction is started with all reactions, all products, or a mixture of both. conc of reactant + product are constant at equilibrium but not equal. Equilibrium position: proportion of reactant + product in equilibrium mixture predominantly products- lie to the right predominantly reactants- lie to the left.

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Related Questions

4. Consider the following: 2NH_3(g) â N_2(g)+ 3H_2(g)

A flask is initially filled with NH₃. As the system approaches equilibrium, the rate of the forward reaction

A. Increases as the rate of the reverse reaction decreases

B. Decreases as the rate of the reverse reaction increases

C. Increases as the rate of the reverse reaction increases

D. Decreases as the rate of the reverse reaction decreases

5. A system at equilibrium is said to be dynamic because at equilibrium the

A. Temperature does not change

B. Macroscopic properties are constant

C. Forward and reverse reactions continue to occur

D. Concentrations of reactants and products are constant

6. In all systems at equilibrium, the

A. Concentration of reactants is less than the concentration of products

B. Concentration of reactants and the concentration of products are equal

C. Concentration of reactants is greater than the concentration of products

D. Concentration of reactants and the concentration of products are constant

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