Kinetics Report.docx - 1 Anikalea Keliiheleua 10 April 2020...

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1 Anikalea Keliiheleua 10 April 2020 Kinetics A rate law is used to explain a rate of change depending on reactant concentrations. Rate laws are written as Rate = k [ A ] x [ B ] y where k is the rate constant that is unique to each reaction, x is the order in respect to the first reactant (A), and y is the order of the reaction to the second reactant (B). The overall order of the reaction is the sum of the exponents in the equation. To determine the order of a rate law, concentrations of one reactant are manipulated while the other remains constant. Then the same manipulation is performed on the other reactant(s). This information is then put into a table and is used to find the order of each reactant, represented by x: Rate 1 Rate 2 x = Concentration 1 Concentration 2 . In the event that molarity cannot be directly measured, The ideal gas law can be used to solve for molarity using pressure V = nRT P . In the reaction 2 H 2 O 2 ( aq ) 2 H 2 O ( l ) + O 2 ( g ) aqueous potassium iodine acts as a catalyst. The release of oxygen causes a pressure change that can be used to determine molarity of reactants. These concepts assist in answering the question: “What is the rate law for the decomposition of hydrogen peroxide?” First, the molar concentration of H 2 O 2 was found from mass and volume of the solution using conversion factors. The conversion resulted in the molar concentration being 0.88

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