The Determination of Keq for FeSCN2+ Joy Muthami February 12 2014 Introduction: The purpose of this lab was to calculate the equilibrium constant for the reaction of iron (III) ions with thiocyanate ions. The materials were first acquired then with the groups in the class each team was given a test solution to create and acquire information from then all the information was put together in order to save time. Specifically the group created test solutions #8‚ #9‚ and #10. Once the solutions were
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names] Section Number: [List 3-digit number] Meeting Time: [Fill in the lab meeting time] TA: [Fill in the lab TA’s name] INTRODUCTION In this experiment I calculated the equilibrium constant for the reaction shown below under different conditions to determine if the equilibrium constant is really constant. Fe3+ (aq) + SCN– (aq) ←→ FeSCN2+ (aq) A big part of this lab includes understanding (and in the end proving) that absorbance is directly proportional to the concentration of a solution
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What is the mysterious dark energy that’s causing the expansion of the universe to accelerate? Is it some form of Einstein’s famous cosmological constant‚ or is it an exotic repulsive force‚ dubbed "quintessence‚" that could make up as much as three-quarters of the cosmos? Scientists from Lawrence Berkeley National Laboratory (Berkeley Lab) and Dartmouth College believe there is a way to find out. | | | | The SuperNova/Acceleration Probe‚ SNAP‚ is a satellite designed to study dark energy
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Determination of Formation Constant‚ Kf of Thiocyanoiron(III)‚ FeSCN+2 Dr. Fred Omega Garces Chemistry 201 Miramar College Chemical Equilibrium: Finding the Formation Constant of FeSCN2+ (aq) Fe3 +(aq) iron(III) + SCN–(aq) FeSCN2+(aq) D thiocyanate thiocyanoiron(III) kf = € FeSCN2 + [ ] Fe +3 [SCN− ] [ ] Objective The purpose of this experiment is to determine the constant formation‚ Kf‚ (equilibrium constant) for the formation of thiocyanoiron(III)
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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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