The Effect of Temperature on the Enzyme Catalase Stephen Francis Biology 183 Abstract This experiment was performed to determine the resultant effect of temperature change on the reaction between the enzyme catalase and hydrogen peroxide. This experiment was performed by measuring and comparing the amount of oxygen bubbles produced and the absorbance of the catalase and hydrogen peroxide solution over time at room temperature‚ 2°C‚ 50°C‚ and 60°C. The overall result of this experiment proved
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B.‚ Choi‚ H.C.‚ and Murugesan‚ V.‚ Solar/ UV-induced photocatalytic degradation of three commercial dyes. Journal of hazardous Materials B‚ (89)‚ 303‚1985. 7. Mozia‚ S.‚ Toyodo‚ M.‚ Inagaki‚M. and Tryba‚B.‚Application of carbon-coated TiO2 for decomposition of methylene blue in a photocatalytic membrane reactor.(2007) 8. Lachheb‚ H.‚Puzenat‚ E.‚ Houas‚ A. and Herrmann‚ J.‚ Photocatalytic degradation of various types of dyes( Alizarin S‚ Crocein Orange G‚ Methyl Red‚ Congo Red‚ Methylene Blue) in water
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knowledge: Enzymes function as biological catalysts‚ increasing the rate of reactions that take place within organisms. Catalase is an enzyme found in the vast majority of organisms that are exposed to oxygen‚ making it very common. It catalyses the decomposition of hydrogen peroxide into water and oxygen. Hydrogen peroxide is a molecule that can attack sulphur atoms and metal ions in protein molecules‚ and with the aid of iron ions is potentionally mutagenic. Catalase is an extremely effective enzyme‚
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Abstract The enzyme peroxidase has been shown to break down H2O2. Enzymes are known to increase the rate at which a chemical reaction occurs. We looked at factors that affected the breakdown of hydrogen peroxide. These effects are the different temperatures and pH levels the enzymes were placed in. We found that the optimum‚ or best condition‚ temperature for the enzymes tested was about 22 degrees Celsius. The optimum pH level for the enzyme was 7. Introduction Enzymes are biochemical that catalyze
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experiments were performed three times‚ where: each compound was mixed with a fixed amount of Fe2+ and various amount of H2O2 and H2O. Solutions were left to react for 3 days‚ and analyzed by size exclusion chromatography and UV-Vis absorbances were taken. In the large scale experiments‚ approximately 100 mg of each compound was mixed with fixed amounts of Fe2+ and H20 and varying h2O2 amounts. They sat until the compound reacted away and were analyzed via size exclusion chromatography. They were then
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Variable Measured How variable was controlled Independent Variable: Temperature (⁰C) of the catalase and H2O2 Both of the solutions will be poured into test tubes/beakers and then cooled and heated to certain temperatures (10‚ 22‚ 30‚ 37‚ 45‚ and 60⁰C) and with the use of ice and a water bath ( in a separate beaker) I attempted to control the temperature of the catalase mixture as well as the H2O2 solution Dependent Variable: Rate of reaction (cm3/second) The gas syringe (± 0.5) is used to measure
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The 22.5% (6.615M)‚ 27% (7.938M)‚ and 30% (8.8M) H2O2 concentrations produced more than 50 mL of O2 and could not be measured past 75 seconds (figure 3.1). There is a drop in initial reaction velocity of 0.065 mL/s between 27% and 30% substrate concentration (figure 3.2). The substrate concentrations
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11.2012 Dr. Charles J. Horn Abstract: This two part experiment is designed to determine the rate law of the following reaction‚ 2I-(aq) + H2O2(aq) + 2H+I2(aq) + 2H2O(L)‚ and to then determine if a change in temperature has an effect on that rate of this reaction. It was found that the reaction rate=k[I-]^1[H2O2+]^1‚ and the experimental activation energy is 60.62 KJ/mol. Introduction The rate of a chemical reaction often depends on reactant concentrations‚ temperature
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room temperature‚ then we will add 5ml of H2O2 and quickly stopper the flask. While one student continues to swirl the flask‚ the other should observe the volume of oxygen produced‚ after 2ml of gas has been evolved. The recordings should be written down at 2ml intervals until 14ml of oxygen has been evolved. Next‚ we will repeat the experiment (making sure everything is the same‚ including the temperature of the bath water) by adding 10ml of KI and 10ml of H2O2 (after swirling the flask)‚ then quickly
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the order of reaction with respect to [H2O2] and [2I-]. I aim to find out the activation enthalpy of the reaction by finding the rate of reaction at different temperatures using the Arrhenius Equation. The experiment will go as follows: Into a conical flask put 15cm3 of distilled water and add 2cm3 of [X]moldm-3 potassium iodide (KI) solution and 1cm3 of 2moldm-3 sulphuric acid. Then add to this 2.5cm3 of 5vol (0.42moldm-3) hydrogen peroxide (H2O2). For the second part of my investigation
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