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CHEM 142 Study Guide - Midterm Guide: Equilibrium Point, Fetal Hemoglobin, Equilibrium Constant

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bluemosquito338

30 Mar 2017

School

Emory University

Department

Course

Professor

Nicholas Llewellyn

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Document Summary

Reversible: a reaction that can proceed in both the forward and reverse directions. Dynamic equilibrium: the condition in which the rate of the forward reaction equals the rate of the reverse reaction. Equilibrium constant (k): the ratio at equilibrium of the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients. Law of mass action: the relationship between the balanced chemical equation and the expression of the equilibrium constant. Kp: as the equilibrium constant with respect to partial pressures in atmospheres. The equilibrium constant, k expresses the relative concentrations of the reactants and the products at equilibrium. Most chemical reactions are reversible; they can proceed in either the forward or the reverse direction. When a chemical reaction is in dynamic equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, so the net concentrations of reactants and products do not change.

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Related Questions

Which one of the following statements is false? a. At equilibrium, the concentrations of the products and reactants are constant. b. At equilibrium, the reaction in the forward direction and the reaction in the reverse direction proceed at the same rate. c. The equilibrium constant is equal to the ratio of the rate constant of the forward reaction over the rate constant of the reverse reaction. d. At equilibrium, the reaction has completely stopped. e. The equilibrium constant for a reaction will change if the temperature changes.

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

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