Kinetics Lab Report.pdf - Part A - Blue -6​ 1. %T​1​ = 5.8...

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Part A - Blue 1.%T1= 5.8 %, Absorbance1 = 1.2366, C1 = 8.9607 x 10-6M 2.%T2= 5.6 %, Absorbance 2 = 1.2518, C2= 6.84 x 10-6M 3.%T3= 5.8 %, Absorbance 3 = 1.2366, C3= 8.9607 x 10-6M 4.Mean Concentration = 8.254 x 10-6M Part A - NaOCl 1.w/w % Stock NaOCl solution - 10 % 2.Molarity of Stock NaOCl Solution - 1.343 M 3.Stock solution used - 5 mL 4.Molarity of Experimental Solution - 0.1343 M Part B Percent Blue Percent NaOCl Time to Colorless (min) 80 % 20 % 16, 14.75 70 % 30 % 15 60 % 40 % 5.66 50 % 50 % 5.5, 5.417 40 % 60 % 2.75 30 % 70 % 2.5 20 % 80 % 2, 1.75 Part C 1.Order of Reaction with Respect to Blue = 1 2.Slope of ln(C)C= -5.57x10-3 3.Kobs = -5.57x10-3 Part D 1.Slope of ln(C)D= -2.57x10-3 2.Order of Reaction with Respect to NaOCl = 1 Results 1.Value of Rate Constant (k) = -0.04147 2.Rate Law = 0.04147[blue]1[NaOCl]1
Kinetics IntroductionIn chemical reactions, identification of reactants and products is fundamental to the understanding of the reaction. However, going past these fundamentals, chemists need to understand how quickly the reactants transform into the products. This is where the study of chemical kinetics comes into frame. Kinetics relates to the measurement and study of rates of reactions in chemistry. This is a fundamental concept for researchers to understand because all research in this field will, in one way or another, involve chemical reactions or reactive properties. Kinetics can be applied to any chemical reaction, from the reaction of combusting gas particles to the dissolving of a solute in a solution. Chemical kinetics has a large number of practical applications. Combustion of gasses, dissolution of gasses or solids in an aqueous solution, decomposition reactions, and all other forms of chemical reactions have specific rates of reaction that can be affected using temperature changes, pressure changes, catalysts, and other

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Term
Fall
Professor
KatieLawrence
Tags
Chemistry, Chemical reaction, Rate equation

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