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CHEM 1301 Chapter Notes - Chapter 14.1-14.6, 16.4 : Dynamic Equilibrium, Equilibrium Constant, Elementary Reaction

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2 Apr 2016

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At the same ime a reacion is consuming reactants, it is also breaking up products: when the amount of products is low, the decomposiion reacion will slow down, and the composiion reacion will speed up. Eventually the rate of decomposiion will equal the rate of composiion and the rate of one reacion exactly balances the other, known as dynamic equilibrium. At dynamic equilibrium the rate of the forward and reverse reacions are equal to each other: dynamic meaning individual molecules react coninuously, equilibrium meaning, there is no net change in the system. If the forward reacion went to compleion, there would be no reactants, if the reverse reacion went to compleion there would be no product, instead we have equal amounts of both. Each the forward and reverse reacions have their own keq. At equilibrium the rates equal each other so we can make. The concentraions you arrange are products over reactants, and we don"t include solids or gases.

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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

EXPERIMENT 5 Don't Get Stressed in the Lab "What a piece of work is a man! How noble in reason! How infinite in faculty! In form and moving how express and admirable! In action bow like an angel! -Hamlet 2.2 Hamlet's awe of humans is no wonder when one considers the amazingly complex intricacies of life. Chemical interactions are constantly taking place within us, regulating, maintaining, and adapting to change. We exist continually in a delicate state of balance between our internal components and the environment. For example, iron aids in the transport of oxygen to the body, which is essential for life. Red blood cells contain hemoglobin, which is a protein that is bound to iron. It is the iron that allows an oxygen molecule to attach to the hemoglobin in order to transport oxygen throughout the body. When the body experiences a deficiency in iron, the amount of oxygen being transported to the body is reduced. Therefore, the body is not able to function at full capacity, resulting in shortness of breath, dizziness, etc. This is called iron deficiency anemia. In order to increase the amount of iron in the body, doctors suggest eating foods high in iron, such as eggs and lean meats. However, people suffering with chis disease are also made aware chat the absorption of firon into the body is dependent on the extent to which iron remains soluble. Iron is easily absorbed when present in acidic conditions. Therefore, intake of iron with orange juice that contains ascorbic acid will increase the intake by the body. (The ascorbic acid also keeps iron in the +2 state which is more soluble.) Once enough iron has been taken in by the body an equilibrium is once again reached. The phenomena of chemical equilibrium is taking place all around us.Chemical equilibrium is never static; it is in constant motion. That motion is a balance between the rate of the forward reaction with the rate of the reverse process. This dynamic equilibrium is the result of the chemical reaction simultaneously producing products while also reverting back to reactants at an equal rate. The mol- ecules are constandy changing; therefore, being dynamic; however, being at equilbrium means the concentrations of the products and reactants have stopped changing.