CHEM 203 Study Guide - Midterm Guide: Reagent, Rate Equation, Reaction Rate Constant

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amaranthdonkey808

20 Apr 2019

School

University of Calgary

Department

Chemistry

Course

CHEM 203

Professor

Bronwen Wheatley

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Document Summary

Large k this is only useful at eq "m. K (cid:8869) doesn"t need to be at equilibrium. Reactants (cid:8869) can be partial pressures or concentrations must be @ eq "m ! usually q is heading towards if q > k reach if q s k forward takes to reverse rxn rxn over. K equilibrium to reach equilibrium (cid:8869) use q to gauge which way eq"m "s going: we don"t use liquids or solids in. Rate of the reaction (cid:8869) [ i / time. = coeft. fi#i=cotefi. xiiidt: slopes f (cid:8869) just rate of reaction for one reactant or one product (cid:8869) need to apply the coefficients. [ rct ] affects the rate of the reaction round to get. Theory: elementary steps / reactions (cid:8869) sum together find the (cid:8869) can intermediates for the overall reaction (cid:8869) the coefficients are. To find out order and catalysts true for k ) orders the.

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

Learning Goal:

To determine equilibrium concentrations from initial conditions.

The reversible reaction

XY(aq)âX(aq)+Y(aq)

has a reaction quotient Qc defined as

Qc=[X][Y][XY]

Because the reaction is reversible, both the forward and reverse reactions will occur simultaneously. The reaction will eventually reach equilibrium, at which point the concentrations do not change, and Qc is equal to a constant known as Kc.

Part C

Based on a Kc value of 0.180 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

CHEM 203 Study Guide - Midterm Guide: Reagent, Rate Equation, Reaction Rate Constant

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