Abstract The aim of this study was to test the rate of reactivity of the enzyme catalase on hydrogen peroxide while subject to different concentrations of an inhibitor. The hypothesis was that hydrogen peroxide will be broken down by catalase into hydrogen and oxygen‚ where a higher concentration of inhibitor will yield less oxygen‚ resultant of a lower rate of reaction. Crushed potato samples of equal weight were placed in hydrogen peroxide solutions of various temperatures. The results showed
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examined and observations were recorded. 8. The samples reacted with chemicals were disposed in the special disposal Erlenmeyer flask provided by the teacher. Samples were recollected as stated in the first procedure. 9. 5 drops of NaOH and 5 drops of CuSO4 were added to each test tube. The Biuret reagent was made by the mixing of two chemicals. 10. The reaction with Biuret reagent was observed and recorded. 11. The solutions were disposed as stated in the 8th procedure; the lab equipment and chemicals
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EXPERIMENT-1 CHEMICAL REACTIONS AIM: To perform and observe the following reactions and classify them into: (i) Combination reaction (action of water on quick lime) (ii) Decomposition reaction (action of heat on ferrous sulphate crystals) (iii) Displacement reaction (iron nails kept in copper sulphate solution) (vi)Double decomposition reaction (reaction between sodium sulphate and barium chloride) APPARATUS REQUIRED: 1. A rack of at least six clean test tubes and a boiling
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have a strong attraction to water. The scientist Irving Langmuir observed a strong repulsive force between hydrophilic surfaces. To dehydrate hydrophilic surfaces—to remove the strongly held layers of water of hydration—requires doing substantial work against these forces‚ called hydration forces. These forces are very large but decrease rapidly over a nanometre or less. They are
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state | Added sodium hydroxide | NaOH (aq) | small blue-ish chunks form | CuOH (s)copper hydroxide | clumps into blue-ish chunks | Added heat (removes H2O) | none | solution becomes muddy black-ish | CuO (s)copper oxide | heated into small‚ black‚ metallic almost shards | Added sulfuric acid | H2SO4 (aq) | turns shards and liquid blue-ish color | CuSO4 (aq)copper sulfate | joins the sulfate after filtering | Added zinc | Zn (s) | small‚ orange‚ metallic shards form in blue
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Conclusion: (Identity‚ % error‚ other evidence‚ how to improve) The identity of Unknown A is the compound cobalt(II) chloride hexahydrate (CoCl₂•6H₂O).This is justified by the similarities in color of red-purple crystal like grains‚ which is significant in identifying the product out of the eight suggested identities. Only two had similar characteristics which were CoCl₂•6H₂O and CoSO₄•6H₂O. Before unknown A was heated‚ there was a notable common physical property of the substance being red crystal
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coming‚ didja) and had a metallic luster. The copper was put in the flame of a Bunsen burner and after several seconds‚ it began to blacken. The flame was applied to it for about a minute and a half‚ and the copper appeared silvery under intense heat‚ but when it was removed from the flame‚ the silver color quickly faded. The copper strip was now black all over‚ and the change in color
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create an endothermic reaction; it absorbs heat and the temperature of the solution falls to about 35 degrees
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know whether a reaction occurred or not. To complete our mission‚ we need to observe carefully some signs of chemical reaction’s appearance such as the change in color of solution‚ precipitate’s existence‚ the release of gas‚ also check the change of heat and light. b) secondly‚ we need to have knowledge about 5 types of reactions and then put experiments below into practice classify type of each reaction. Furthermore‚ we also learn how to describe chemical changes carefully‚ beside that we will
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recorded; the change in temperature (∆T) was calculated by subtracting the initial temperature from the final temperature. The reaction was performed twice for every calorimeter. The heat capacity (Ccal) of each calorimeter was calculated using the formula‚ C_cal=(-〖∆H〗_rxn^o n_LR)/∆T [1] where ∆Horxn is the total heat absorbed or evolved for every mole of reaction and nLR is the number of moles of the limiting reactant. The ∆Horxn used was -55.8kJ per mole of water while the nLR was 0.005 mole
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