NATURE OF THE EQUILIBRIUM STATE: Equilibrium is the state where the rate of the forward reaction is equal to the rate of the reverse reaction. At these conditions‚ concentrations of all reactants and products remain constant with time once equilibrium has been established at constant temperature. (In stoichiometry‚ we dealt with equations that went to completion; often equilibrium equations are going to fall short of this goal.) Reactions are reversible. This is indicated by double arrows. • dynamic--
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Experiment 3: Chemical Equilibrium Purpose The purpose of this experiment was to determine the equilibrium constant for the formation of FeSCN2+. Introduction Chemical equilibrium is the point in a reversible reaction where the concentration of the reactants and that of the products remains constant. This point of equilibrium is referred to as the Kc value‚ which can be obtained using the formula: Kc = [product] [reactant] In this experiment‚ we used a spectrophometer to
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experience the meaning of equilibrium. 3. How did the calculated ratios of product to reactant compare in the three parts of this activity. Explain‚ in paragraph form‚ if these ratios illustrate the concept of the law of mass action and the equilibrium constant of a system. 4. What determines when a system reaches equilibrium? What observations can be made about a system once equilibrium has been established? The rate of the forward reaction must equal to the
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Ratio and Proportion • If 2 numbers are in ratio a: b then consider them as ax and bx (where x is the proportionality constant) and apply ax and bx in the given condition of the problem to proceed for answer • Ratio can be applied between 2 units if and only if the same physical quantity is compared • Length : length is correct • Length : density is wrong • Ratio can be made only after the units are compared in the same unit • If two lengths are 1 mile and 1 km respectively then ratio
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Chapter 4 Applications of First-order Differential Equations to Real World Systems 4.1 Cooling/Warming Law 4.2 Population Growth and Decay 4.3 Radio-Active Decay and Carbon Dating 4.4 Mixture of Two Salt Solutions 4.5 Series Circuits 4.6 Survivability with AIDS 4.7 Draining a tank 4.8 Economics and Finance 4.9 Mathematics Police Women 4.10 Drug Distribution in Human Body 4.11 A Pursuit Problem 4.12 Harvesting of Renewable Natural Resources 4.13 Exercises In Section 1.4 we have seen that
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equilibrium constant of the iron thiocyanate complex could be determined. In order to accomplish these tasks‚ five different solutions were made. Upon completion of the experiment‚ the results of the aforementioned experiments were calculated to an average of the final formation constant of 183. Introduction: The experiment for the Spectrophotometric Determination of Equilibrium had the main objectives of determining the position of equilibrium and the formation of the equilibrium constant of the
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system to be in the state of dynamic equilibrium. (4 points) Dynamic equilibriumis a state of balance where the forward and the reverse reactions occur at the same time and the rates are the same. The reverse reaction and forward reaction are kept constant with time. Only closed systems have equilibriums. 2. Describe what you observed in each part of this lab. Do you think that each part of this activity helped to illustrate the concepts of equilibrium? Explain your answer completely in paragraph
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Spectrophotometric determination of the equilibrium constant of a reaction K.F.P. Boado Department of Chemical Engineering‚ College of Engineering University of the Philippines‚ Diliman‚ Quezon City‚ Philippines 4 March 2015 Jade Nazareno ABSTRACT The experiment aims to determine the Keq of the formation of Fe(SCN)2+ through the use of UV-Vis spectrophotometry. The solutions used in the study were allowed to equilibrate days before calibration in a UV-Vis spectrophotometer which determined the absorbance
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change in chemical equation with a new equilibrium constant. An overall reaction is the sum of two or more reaction steps with different equilibrium constants. The overall equilibrium constant‚ Koverall‚ is the product of the equilibrium constants of the individual reaction step. If a reaction step is reversed‚ the equilibrium constant is set into its reciprocal. If a reaction step is multiplied by a common coefficient n‚ the new equilibrium constant is raised to the nth. The first part of the experiment
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react with thiocyanate ions (SCN-) to form iron (III) thiocyanate‚ FeSCN2+. It is represented in the equation below: Fe3+ (aq) + SCN- (aq) FeSCN2+ (aq) Therefor the equilibrium constant for this reaction is: KC = [FeSCN2+]/([Fe3+]•[SCN-] For this experiment we were able to determine the equilibrium constant KC for this reaction. First we prepared five different mixtures with known initial concentrations of iron (III) and thiocyanate ion. By using the colorimeter we determined the absorbance
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