The kinetics of the Harcourt-Essen Reaction (Hydrogen peroxide variation) Aims: To find the order of the reaction with respect to the Hydrogen Peroxide (H2O2)‚ Potassium Iodide (KI) and the Sulphuric Acid (H2SO4) by the use of an Iodine clock reaction. Calculate the rate constant‚ mechanism and equation Find the effects of temperature on the rate of reaction The effects of a catalyst on the rate of reaction Find the activation enthalpy (Ea) of the reaction‚ with and without a catalyst Background:
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material elements in contact. It is usually subdivided into several varieties: * Dry friction resists relative lateral motion of two solid surfaces in contact. Dry friction is also subdivided into static friction between non-moving surfaces‚ and kinetic friction (sometimes called sliding friction or dynamic friction) between moving surfaces. * Lubricated friction or fluid friction resists relative lateral motion of two solid surfaces separated by a layer of gas or liquid. * Fluid friction
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The kinetic theory of gases describes a gas as a large number of small particles (atoms or molecules)‚ all of which are in constant‚ random motion. The rapidly moving particles constantly collide with each other and with the walls of the container. Kinetic theory explains macroscopic properties of gases‚ such as pressure‚ temperature‚ or volume‚ by considering their molecular composition and motion. Essentially‚ the theory posits that pressure is due not to static repulsion between molecules‚ as
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The halides in unknown solution were identified as iodide and chloride based on their experimental E°(Ag/AgX) values‚ -0.16 ±0.01V and 0.22 ±0.02V respectively. These results were both accurate with percent error of 5.96% for iodine and 0.9% for chloride. The literature value of E°(Ag/AgI) and E°(Ag/AgCl) were -0.151V and 0.222V respectively (1). In addition‚ the literature vales lay within the 95% confidence interval for both halides therefore the results were accurate. These results were precise
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BIOCHEMISTRY 304 Enzyme Kinetic Sample Problems #1 September 2004 1 Given the reaction k1 kp E + S ES E + P k-1 where k1 = 1 x 107 M-1 sec-1 k-1 = 1 x 102 sec-1‚ and kp = 3 x 102 sec-1 a) Calculate Ks b) Calculate Km (a) k-1 1 x 102 sec-1 Ks = k1 = 1 x 107 M-1 sec-1 = 1 x 10-5 M (b) k-1 + kp (1 x 102 sec-1) + (3 x 102 sec-1)
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Lecture No. 1 Chemical Kinetics 1.1 The Rate of a Reaction Chemical Kinetics is the area of Chemistry that is concerned with the speed‚ rate or mechanism at which a chemical reaction occurs. Reaction Rate is the change in the concentration of a reactant or product with time (i.e. M/s). It measures how fast a reactant is consumed and how fast a product is formed. 1.2 WRITING RATE EXPRESSIONS Consider the following hypothetical reaction. A + 2B ( 3C + D Rate = - rate
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Enzymes are naturally occurring biological catalysts that are extremely efficient and specific. Enzymes accelerate the rate of a reaction by factors of at least a million as compared to the same reaction without the enzyme. Most biological reaction rates are not perceivable in the absence of the enzyme. The term enzyme was first used by a German pshysiologist Wilhelm Kühne in 1897. There are over 700 different kinds of enzymes that have been identified. Enzymes can be classified into several categories
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Enzyme Kinetics Marcos‚ Nelissa S. Institute of Chemistry‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines ABSTRACT The rationale of the experiment is basically founded in the concept of reaction rates as affected by enzyme‚ and how the enzyme works is competed by a competitive inhibitor‚ thereby impeding the forward reaction. In this experiment‚ o-diphenol oxidase‚ an enzyme that causes the browning in fruits‚ was extracted from banana and reaction rate of this was established
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using ammonium persulfate Assessment criteria: Design Variables: Table 1.1: List of dependent and independent variables. S.No | Dependent variables | Independent variables | Controlled variables | 1. | Rate of reaction | Temperature | Concentration | 2. | - | - | Pressure | 3. | - | - | Volume | Hypothesis: The iodine clock reaction is an experiment that demonstrates chemical kinetics in action. The iodine
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Use the knowledge of kinetics to explain each of the following statements. a. An increase in temperature at which a reaction takes place causes an increase in reaction rate . An increase in temperature means increasing the energy of the molecules present. If the molecules has more energy ‚ then more of the them will collide often with enough energy ‚ to overcome the activation energy barrier. causing the reaction to proceed more quickly. b.An addition of the catalyst increases the rate at which
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