CHE 132 Lecture Notes - Lecture 8: Rice Chart

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viridianhare340

14 Feb 2019

School

Stony Brook University

Department

Chemistry

Course

CHE 132

Professor

Fernando Raineri

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CHE 132 Lecture 7: CHE 132 Lecture 7

CHE 132 Lecture Notes - Lecture 8: Rice Chart

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This can be seen by the stoichiometric coefficients. Write an x after each number as well. The sign of these numbers will determine if the reaction will go forward or reverse. If it goes forward, then the reactants side will be negative and products side positive. This is because you are making more products and getting rid of reactants. If the reaction is at equilibrium then grxn = 0. If there are too many reactants then grxn < 0 and the reaction will go forward. If there are too many products then grxn >0 and the reaction will go in the reverse. Q > k: a very small q = - grxn.

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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

Le Chatelierâs principle describes the way that a reaction atequilibrium will respond if that equilibrium is somehow disturbed.Imagine that you have a reversible reaction you want to performthat produces a very valuable product but the equilibrium constantfor the process is very low. Using the 3 definitions of equilibriumpresented in lecture as your framework, explain in no more than 1paragraph how the yield of reaction can be greatly increased(meaning reactants are more extensively converted into products) byapplying Le Chatliers principle.

The 3 definitions we learned in lecture:

1. rate of forward reaction= rate of reverse reaction

2. no observable change in [reactants] or [products]

3. no change in energy

I know that Le Chatliers principle states that if a system atequilibrium is disturbed, then the system will adjust so thatequilibrium can be established. I also know that if reactants aresuddenly added to a reaction already at equilibrium, then potentialenergy has effectively been added to reactant side vs. product sideof reaction. Since the system has been pushed to a higher levelthan what would be experienced at equilibrium, the reaction willproceed forwards until the lowest energy point (equilibrium) hasbeen reached. I am not sure though if this is the answer myteacher is looking for.

Does this make sense?

CHE 132 Lecture Notes - Lecture 8: Rice Chart

CHE 132 Lecture 7: CHE 132 Lecture 7

CHE 132 Lecture Notes - Lecture 8: Rice Chart

CHE 132 Lecture 9: CHE 132 Lecture 9

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