Determination of the Equilibrium Constant for Ferric Thiocyanate In this laboratory exercise‚ the equilibrium constant(Kc) for the reaction between the Ferric Ion (Fe3+) and the Thiocyanate Ion (SCN-) was determined. After measuring the absorbance of the Ferric Thiocyanate‚ and carrying out some calculations; it was determined that Kc=130.81M Introduction: Chemical equilibrium is established when a reaction exists in a state where the forward reaction rate is equal to its reverse reaction
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DATE PERFORMED: JULY 20‚ 2007 SPECTROPHOTOMETRIC DETERMINATION OF EQUILIBRIUM CONSTANT FOR A REACTION ABSTRACT UV-VIS spectrophotometry is one of the most widely-used methods for determining and identifying many inorganic species. During this experiment‚ this spectrophotometry was used to determine the equilibrium constant‚ Keq‚ of the Fe3+(aq)+SCN-(aq)↔ FeSCN2+(aq) reaction. By determining the amount of light absorbed‚ the concentration of the colored FeSCN2+ solution was also quantitatively
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Date Performed: January 10 & 15‚ 2013 Spectrophotometric Determination of the Equilibrium Constant of a Reaction R.J.V. Ortega and J.C.V. Gatdula Institute of Chemistry‚ College of Science University of the Philippines‚ Diliman‚ Quezon City‚ Philippines Received January 22‚ 2013 ------------------------------------------------- ------------------------------------------------- ------------------------------------------------- ABSTRACT -------------------------------------------------
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- All firms are price takers - All firms have a relatively small market share - Buyers know the nature of the product being sold and the prices charged by each firm. - The industry is characterised by freedom of entry and exit. Perfect competition is a theoretical market structure. It is primarily used as a benchmark against which other market structures are compared. The industry that best reflects perfect competition in real life is the
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Test Version A SEMESTER I EXAMINATIONS Mid-Term Assessment ECON 30110 Microeconomics II Time Allowed: 50 minutes Instructions for Candidates This exam counts for 30% of the Module Grade. All questions carry equal marks. Note there is NO negative marking Correct answer is worth 1 mark. No answer or more than one answer‚ will both receive a 0 mark. Incorrect answer will receive a 0 mark. Attempt all 20 questions. Shade in the box in the appropriate space with
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The Equilibrium Constant of an Ester Hydrolysis Reaction Julia Stanley CHM 152 LL Dr. Asmita Kane Budruk Goal of the lab: The purpose of this laboratory is to determine the equilibrium constant‚ Kc‚ for the acid-catalyzed reaction between an unknown ester and water to produce an unknown alcohol and an unknown carboxylic acid. I was using Unknown Ester #3 with a density of 0.9342 and Molar Mass of 74.08 g/mol; alcohol with density 0.7914 and Molar Mass 32.04 g/mol. Chemical
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Obviously this is all in the short term‚ but if we wish to find it with terms of market value we would time the equation by the price so say our good is p=100 we get‚ Q=P(10K^0.5L^0.5) so with ours we get Q=100(10K^0.5L^0.5)=1000K^0.5^0.5 giving us the firms total revenue in term of sale price and labour and capital the firm hires. Equilibrium price and output for the industry‚ and the effect on the equilibrium of an imposition of an ad valorem tax‚ in relation to Cobb Douglas. A perfectly
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Hardy-Weinberg Equilibrium One of the most difficult concepts to understand about the process of evolution is how changes in the genetic composition of a population affect the phenotypic composition of a population‚ and how both ultimately act to allow evolution of the species. Charles Darwin’s theory of evolution emphasizes that populations‚ not individuals‚ evolve. The purpose of my experiment was to test the allele and genotype frequencies. Alleles for a gene are represented by letters of
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General Chemistry II Determining of the equilibrium constant for the formation of FeSCN2+ Introduction The objective of this experiment was to determine the equilibrium concentration and then determine Kc. A dilution calculation was formed to determine the concentration of SCN- and Fe(SCN)2+. Each cuvette was filled to the same volume and can be seen in table 1. Then the absorbances were recorded from each cuvette and can be seen in table 1. A Beer’s law plot was made from the data that was recorded
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LIST OF TABLES |Serial No. |Name of the Table |Page No. | |1 |Classification Of Respondents On The Basis Of Age |29 | |2 |Classification Of Respondents On The Basis Of Sex |30 | |3 |Classification
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