concentration‚ temperature‚ surface area and catalyst on the rate of chemical reactions. The nature of the reactants implies a difference if the reactants are aqueous or organic‚ acidic or basic or if they occur in the same phase or not. Acid-base reactions‚ formation of salts‚ and exchange of ions are fast reactions while reactions in which large molecules are formed or broken apart are usually slow. Generally‚ the rate of reaction is directly proportional to the concentration of the reactants
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varying the concentration of H2O2 has on the reaction‚ and to determine the respective order of reaction. To investigate the effect of varying the concentration of KI has on the reaction‚ and to determine the respective order of reaction. To investigate the effect of varying the temperature has on the reaction‚ and to determine the respective order of reaction. To investigate the effect of introducing Ammonium Molybdate to the reaction Arrhenius stuff The reaction of Hydrogen Peroxide and Iodide
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Reaction Mechanisms The mechanism of a chemical reaction is the sequence of events that take place as reactant molecules are converted into products. Introduction The study of kinetics includes very complex and sophisticated reactions that cannot be analyzed without a proposed mechanism‚ a series of steps that a reaction takes before reaching the final products. Reaction mechanisms are step-by-step descriptions of what occurs on a molecular level in chemical reactions. Each step of the reaction
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PM Introduction: This experiment was conducted to examine the breakdown of substrate hydrogen peroxide (H2O2) by catalase‚ which is a specific enzyme that breaks down substrates of (H2O2). Molecules are in our bodies and nature. They move around constantly which causes them to be part of random collisions‚ which produce chemical reactions. This is actually needed to sustain life. These collisions are influenced by many different physical factors‚ such as temperature or
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CHM1022 Lab Report 1 Rate Law of an Iodine Clock Reaction Name: Sashini Naomi Wijesekera Student ID: 23877847 Lab Partner: Zahiya Imam Lab Session: Monday 9.00am Aim The aim of the experiment is to determine the factors that affect the rate of a reaction‚ by performing the iodine clock reaction and repeating it changing different initial conditions in order to measure and compare the rate of reaction for each experiment and experimentally
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Introduction Enzymes are proteins produced by living organisms to speed up the rate in which chemical reactions occur. This process can happen fast‚ slowly‚ or stop the chemical reaction all together depending on the temperature‚ pH and concentration. Catalase is one of the most common enzymes. It is found in living organisms and is used to break down hydrogen peroxide. This must happen because hydrogen peroxide is considered toxic to cells in the body. However‚ when catalase is used it breaks
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Investigating the Kinetics of the reaction between Iodide ions and Peroxodisulphate (VI) ions By the use of an Iodine clock reaction I hope to obtain the length of time taken for Iodine ions (in potassium iodide) to react fully with Peroxodisulphate ions (in potassium Peroxodisulphate). I will do three sets of experiments changing first the concentration of iodide ions‚ then the concentration of Peroxodisulphate ions and finally the temperature of the solution in which the reaction is taking place. From these
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Many organisms can decompose hydrogen peroxide (H2O2) enzymatically. Enzymes are globular proteins‚ responsible for most of the chemical activities of living organisms. They act as catalysts‚ substances that speed up chemical reactions without being destroyed or altered during the process. Enzymes are extremely efficient and may be used over and over again. One enzyme may catalyze thousands of reactions every second. At the start of the reaction‚ there is no product‚ and the concentration is the
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concentration of the hydrochloric acid and the rate of a reaction. To find this out I will react different concentration of hydrochloric acid and magnesium‚ from there I will monitor the gas (hydrogen) produced and analyse the results. Prediction: I predict the higher the molarity of the hydrochloric acid the faster the rate of reaction therefore the quicker the gas will be produced in the specific time interval. Overview of the experiment: In this reaction two substances will be present in the
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hydrogen peroksida secara sedehana: H2O2 -> H2O + 1/2O2 + 23.45 kcal/mol Pembahasan H2O2 Hidrogen peroksida dengan rumus kimia H2O2 ditemukan oleh Louis Jacques Thenard di tahun 1818. Senyawa ini merupakan bahan kimia anorganik yang memiliki sifat oksidator kuat. Bahan baku pembuatan hidrogen peroksida adalah gas hidrogen (H2) dan gas oksigen (O2). Teknologi yang banyak digunakan di dalam industri hidrogen peroksida adalah auto oksidasi Anthraquinone. H2O2 tidak berwarna‚ berbau khas agak keasaman
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