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Chemistry 1027A/B Study Guide - Final Guide: Amide, Aldehyde, Van Der Waals Strain

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apricotsheep340

8 Dec 2013

School

Western University

Department

Course

Chemistry 1027A/B

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Document Summary

Reversible chemical reactions at equilibrium, system contains both reactants and products (dynamic) Equilibrium achieved when rate of forward reaction = rate of reverse. At the molecular level, both forward and reverse processes are still occurring. Equilibrium constant (k) is the mathematical relationship between pressures. Concentration of pure solids and liquids are not included in k. Numerical value of k only changes if the temperature of the system changes. Same phase = homogenous / different phase = heterogeneous. Magnitude of the equilibrium constant is an indication of the relative amount of product / reactant. If k is large more products are present, equilibrium lies to the right. If k is small more reactants are present, equilibrium lies to the left. Reaction quotient (q) indicates whether or not the system is at equilibrium and the direction in which the reaction must proceed. Q < keq: reaction must proceed in forward direction (not enough product)

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Related Questions

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.

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