this experiment was to use Iodine‚ Benedict and Biuret to test the reaction of the following 12 samples: 1% glucose‚ 0.3% glucose-1-phosphate‚ 1% maltose‚ honey‚ 1% sucrose‚ 1%lactose‚ 1% glycogen‚ 1% starch‚ protein‚ beer‚ distilled water and an unknown solution (test tube: 300). The iodine test for starch was to test how would starch reacted if we put iodine in it. The color of starch before the test was clear. The color of the iodine was brown. When you added iodine into starch‚ the result was
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SCHOOL OF FOOD SCIENCE & NUTRITION LABORATORY REPORT NT20903 FOOD CHEMISTRY AND BIOCHEMISTRY Determination of free fatty acid(FFA) and iodine value (IV)in oil LECTURER NAME : MOHD NAZRI BIN ABDUL RAHMAN LAB SESSION : 3 OCTOBER 2011 (GROUP 4‚ MONDAY) Group Member Title: Determination of free fatty acid (FFA) in oil and determination of iodine value (IV) in oil Introduction Acid value or free fatty acid content is an important characteristic commonly used in quality control of fat
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reaction progresses‚ showing how the concentration of Iodine changes with time and how varying concentrations of KI and H2O2 solutions affects the rate of reaction. 2 - Use an iodine clock: add 2cm3 of 0.1moldm-3 sodium thiosulphate (Na2S2O3) and 1cm3 of 1% starch solution at the start of the reaction. The added sodium thiosulphate reacts with the iodine as it’s formed: I2 + 2Na2S2O3 -> 2NaI + Na2S4O6 When the sodium thiosulphate is all used up the iodine remains in solution and reacts with the starch
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Effect of Iodine on mercury concentrations in dental-unit wastewater John Michael Panganiban and Ian Jasper Ocampo Objective: This study was undertaken to determine whether iodine used to control bacteria in dental unit wastewater could increase mercury concentrations in dental wastewater. Introduction: Two of the major concerns in dentistry are biofilm in dental unit waterlines and the contamination of dental unit wastewater with mercury. Biofilms are microscopic communities that consist
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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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Lab : Iodine-starch Clock Reaction Pre-lab: Before the lab was conducted‚ the concentration of the Iodate ions to be in the mixture made by dissolving specific volumes of solution A with a constant concentration and water was calculated using the dissolution formula: C1V1 = C2V2 Sample Calculation 1: Concentration of the Iodate ions: For mixture 1: C2 = C1V1/ V2 = (0.020mol/L) x (0.003L)/(0.01L) = 0.006mol/L The same calculations were used in the calculating of the
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Due to the lack of literature value for the effects of temperature on the rate of the Iodine Clock Reaction‚ there was no final percentage error. However‚ Looking at Graph 1.6‚ the line of best fits clearly shows the low precision throughout this experiment resulting in an increase of Random error. This could be due to the many assumptions
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Purpose: To determine the general rate law for the reaction of S2O82- + I- through a series of experiments and calculations. Materials: -Temperature probe -3 large test tubes -3 rubber stoppers -Pipets -0.20 M KI soln -0.20 M NaCl soln -0.010 M Na2S2O3 soln -2% starch soln -0.20 M K2SO4 -0.20 M K2S2O8 -0.2 M CuSO4 -Timer or stopwatch -Small beaker -Hot water Procedure: Refer to Lab #12‚ No changes Data: Table #1: Quantitative/Qualitative Observations Room Temp: 25.4°C
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It was originally hypothesised that the reaction time would decrease with higher concentrations of the reactants‚ potassium iodate and sodium bisulfite as collision theory stated that more molecules present in a given volume meant a greater chance they would collide. Furthermore‚ the time was expected to decrease with higher temperatures as it influenced the reactant particles by raising their kinetic energy. However‚ the data collected from this experiment only partially supported this hypothesis
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Introduction The purpose of this experiment is to determine the rate equation for the “Iodine Clock Reaction” experiment. The experiment will consider the equations 〖2I〗^-+S_2 O_8→2〖〖SO〗_4〗^(2-)+I_2 and I_2+2〖S_2 O_3〗^(2-)→2I^-+S_4 O_6 in order to determine the rate law of Rate=k[〖〖S_2 O_8〗^(2-)]〗^a 〖[I^-]〗^b by using the experimental data to calculate the values of exponents a and b as well as the rate constant k. Experimental Supplies Needed: 250 mL Erlenmeyer flask‚ 100 mL beaker‚ graduated
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