Finding the Activation Energy of the reaction between Hydrochloric Acid and Sodium Thiosulfate The equation for the reaction is: S2O32- (aq) + 2H+(aq) ⋄ SO2 (g) + S(s) + H2O (l) Equipment - 2 boiling tubes - 400 cm3 beakers - Marker pen - Stand and clamp - Timer - Bunsen burner‚ tripod and gauze - 0 – 100 oC thermometer - 2 x 10 cm3 measuring cylinders - Access to a fume cupboard. Method 1. Label two boiling tubes A and B. Mark a dark spot on the side of a 400cm3 beaker‚ then ½ fill
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environments affecting the rate of reaction‚ PNPP (p-nitrophenyl phosphate) + H20 ? PNP (p-nitrophenol) + H3P04. This reaction is catalyzed by the enzyme phosphatase. Different environments produced different reaction rates as environmental factors affect the efficiency of phosphatase. This is because environmental factors can change the tertiary structure of phosphatase‚ which alters its active site‚ and thus changes its efficiency to catalyze the reaction. We measured the rate of reaction‚ by using a chromogenic
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Practical 3 Investigation of Action of Saliva and Hydrochloric Acid in Two Carbohydrate Solution | Objective: 1. To show the action of saliva in two carbohydrate solutions. 2. To show the action of hydrochloric acid in two carbohydrate solutions. Apparatus & Equipment’s: Boiling tubes Metal test tube racks Beaker Graduated plastic dropper Water bath‚~37°C Water bath‚~95°C Stop watch
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Reaction Order and Rate Law Name Data‚ Calculations‚ and Questions A. Calculate the initial and final concentrations as needed to complete Tables 1 and 2. Data Table 1: Varying the Concentration of 1.0 M HCl | | | | |Concentrations | | |# Drops |# Drops |# Drops |Initial
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Determination of Rate and Order of a Reaction Results This experiment used a spectrometer to find the wavelength with maximum absorbance in a green food coloring solution. For this particular solution the wavelength was 629.7 nm. The system was then calibrated to that and was set to measure the food coloring and bleach solution. The measured visible light absorbance of the mixed solution was collected over a time of 200 seconds and eight points were then selected and placed into the Absorbance
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Experiment 4: Analyze a solution of potassium hydroxide using standard hydrochloric acid Theory . Introduction: Titration is a procedure used in chemistry in order to determines the molarity of an acid or a base. In the other words‚ it is also consider as acid-base neutralization reaction (Darrell D. Ebbing 1976). A chemical reaction is set up between a know volume of a solution of unknown concentration and a known volume of a solution with a known concentration. The relative acidity or
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Title: Kinetics: The Rate of a Chemical Reaction Objectives: 1. To study the kinetics of chemical reaction‚ 2 I- + S2 O82- I2 + 2 SO42- . 2. To study the effects of reactant concentration (persulphate‚ S2O82-‚ and iodide‚ I-) and temperature on the rate of chemical reactions. ( i) Study the effect of 0.20M (S2O82-) on the rate of chemical reaction. ( ii) Study the effect of 0.10M (S2O82-) on the rate of chemical reaction. ( iii) Study the effect
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Pre Lab Experiment 8 DETERMINATION OF % COMPOSITION OF PENNIES USING REDOX AND DOUBLE DISPLACEMENT (PRECIPITATION) REACTIONS Objectives: 1. Learn how to determinate the percent composition 2. Learn how to get the percent using oxidation reduction and double reactions 3. To become more familiar with the use titration techniques 4. To learn how to get the salt out of an quimical Background: To develop and utilize procedures to determine the percent composition‚ of ZnCI2. As well titrating
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RESULTS AND DISCUSSION REPORT—EXPERIMENT 3 (CHEMICAL KINETICS) CALCULATIONS Effect of Concentration on Reaction Rate [S2O32-]initand [H+]init for each run‚ knowing the original concentrations and volumes of [S2O32-]‚ [H+]‚ and water used. [S2O32-]init= __(M[S2O32-])(V[S2O32-])__ [H+]init= _____(M[H+])(V[H+])____ V[S2O32-]+V[H+]+V[water] V[H+]+V[S2O32-]+V[water] Run 1 [S2O32-]init= (0.15 M)(10 mL) (10+3+2)mL = 0.1 M [H+]init= (3 M)(2
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Affecting Rate of Reaction Introduction Hydrogen Peroxide (H2O2)‚ is the most simple peroxide and commonly used in several household items such as toothpaste or as an alternative to bleach. However hydrogen peroxide it is a very dangerous substance when accumulated in large amounts. If that situation occurs this substance must be decomposed. But how can we decompose this reaction? Well it decomposes by itself very slowly (2H2O2(aq) -> 2H2O(l) + O2(g))‚ but that would take too long. This reaction can
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