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    AP Chemistry Notes

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    Notes 12.1 The N2O4-NO2 Equilibrium System When you put a sample of N2O4‚ a colorless gas‚ in a closed container at 100C a reddish-brown color starts to show. This is due to NO2 formed by the decomp. of part of the original substance. The forward and reverse reactions are taking place at the same rate. The concentrations of species present remain constant with time. These concentrations are independent of the direction from which equilibrium is approached. The equilibrium constant K is where the

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    Unit 16 Study Guide

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    concerning equilibrium is not true? A) A system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. B) Equilibrium in molecular systems is dynamic‚ with two opposing processes balancing one another. C) The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained. D) A system moves spontaneously toward a state of equilibrium. E) The equilibrium constant

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    Yuyii

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    Position of Equilibrium * There are many equilibrium mixtures possible for a given chemical reaction‚ depending on the concentrations of solutions‚ the pressure of gases and the temperature of the reaction. * The term position of equilibrium can be used to describe a particular set of equilibrium concentrations for a reaction. * If either the temperature‚ pressure or concentration of one of the substances changes‚ then the concentrations of all the substances will change until a new

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    Chem 130 Chp. 15

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    Chp. 15 Chemical equilibrium: Occurs when a reaction and its reverse reaction (opposing reactions) proceed at the same rate At equilibrium the rate at which products are produced from reactants equals the rate at which reactants are produced from products At equilibrium a particular ratio of concentration terms equals a constant The composition of an equilibrium mixture does not change with time Kc: equilibrium constant 15.2 Law of mass action: expresses the relationship between

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    Chemistry Test Questions

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    1) At equilibrium‚ __________. A) all chemical reactions have ceased B) the rate constants of the forward and reverse reactions are equal C) the rates of the forward and reverse reactions are equal D) the value of the equilibrium constant is 1 E) the limiting reagent has been consumed 2) Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (s) + H2O (l) ⇌ H3O+ (aq) + F- (aq) A) [HF][H2O] / [H3O+][F-] B) 1 /[HF]

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    Example of Lesson Plan

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    minutes TITLE: MARKET SUB TITLE: - Market equilibrium - Meaning the market equilibrium - Market disequilibrium OBJECTIVE: At the end of the lesson‚ students will be able to: i) Explain the purpose of market equilibrium ii) Draw a diagram of market equilibrium under the given table iii) To explain the determination of market equilibrium price and quantity based on the tables

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    oligopoly

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    there are two firms A and B. Suppose A wants to produce more. In order to judge whether this decision of increasing production is gainful or not A has to conjecture how B will react to this decision. This is conjectural variation. The nature of the equilibrium changes with change in conjectural variation pattern. In oligopoly firms have several decision variables. It can decide on quantity‚ price‚ quality of product‚ advertisement‚ investments‚ timing of entry in the market etc. Existence of so many

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    msne

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    Mixed Strategy Nash Equilibrium May 22‚ 2012 () Mixed Strategy Nash Equilibrium May 22‚ 2012 1 / 12 Drawback of Pure Strategy Nash Equilibrium One drawback of the pure-strategy Nash equilibrium concept is that it many games do not have a pure-strategy Nash equilibrium. (Rock paper scissors‚ matching pennies to name a couple) Does this mean that we have no solution concept for these types of games? Not by a long shot! () Mixed Strategy Nash Equilibrium May 22‚ 2012

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    Chem Worksheet

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    Question 1 Consider the following equilibrium.4NH3(g) + 3O2(g) | View Full Image | | 2N2(g) + 6H2O(g)Suppose 0.30 mol of NH3 and 0.40 mol of oxygen are added to a 5.0-L container. If x mol of water is present at equilibrium‚ what is the equilibrium concentration of oxygen?Answer 0.40 - 0.50x | 0.30 - 0.50x | 0.08 - 0.10x | 0.06 - 0.13x | 0.40 - | View Full Image | | x | 4 points Question 2 At 298 K‚ the value of Kc for the reaction

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    ib chem past paper

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    The equilibrium law DYNAMIC EQUILIBRIUM forward A +8 reaction ""r=====~’~ reverse reaction Most chemical reactions do not go to completion. Once some products are formed the reverse reaction can take place to reform the reactants. In a closed system the concentrations of all the reactants and products will eventually become constant. Such a system is said to be in a state of dynamic equilibrium. The forward and reverse reactions continue to occur‚ but at equilibrium the

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