The catalytic effect of D-block ions and the kinetics of reactions iodine clock reaction: By Stephen Parsons 6K2 Centre number: 61813 Candidate number: 8270 Table of Contents My aim and my reaction: 3 Rate of reaction: 4 Activation enthalpy: 5 Collision theory: 6 The effect of temperature on reaction rate: 7 The effect of concentration on reaction rate: 7 The effect of a catalyst on reaction rate: 8 D-block elements: 9 The effect of extra kinetic energy (from stirring etc.): 10 Where
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Colleen Hamilton AP Lab 4: Determining the Rate of Cellular Respiration of Peas at Varying Temperatures and Stages of Germination I. Purpose and Intro The purpose of this lab is to determine the rate at which germinating peas respirate at varying temperatures and stages of germination. Cellular respiration is the set of metabolic reactions and processes that takes place in an organism’s cells in order to create ATP from sugar. It occurs in the mitochondria and comprises three stages: glycolysis
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boat to hold and measure the mass. (The weight of the weigh boat was zeroed out prior to measuring the salt). Once we added the salt to the ammonia and completely mixed the solution‚ we pipetted 20 mL into a volumetric flask. Then we set up a titration system using 0.100M NaOH in the buret. For the step-by-step procedure guidelines‚ refer to‚ “Investigations of Buffers. CHM 116 Spring 2013 Lab Manual‚ Grand Valley State University pages 49-56” III. Data Ammonia/Ammonium Buffer
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Table 1 results were determined by pH analysis and EDTA titration. The moles of EDTA was found by using the EDTA concentration of 0.025 mol/L. Table 2. Conductivity probe calibration Figure 1. Conductivity of standard NaCl using conductivity probes. 1"H2OKits.com Water Blog." Negative Effects of Hard Water. H20 Kits‚ 16 Sept. 2008. Web. 11 Oct. 2013. 2”Water Hardness." Water Hardness. Freshwatersystems‚ n.d. Web
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Restoring Balance LeChâtelier’s Principle and Equilibrium Introduction Chemical equilibrium is a true balancing act. What happens when the balance is disturbed? The purpose of this lab is to observe the effects of concentration and temperature on equilibrium and to visualize how balance can be restored based on LeChâtelier’s Principle. Background Not all chemical reactions proceed to completion‚ that is‚ to give 100% yield of products. In fact‚ most chemical reactions are reversible
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Student number: 658184 Due Date: 19th Sept 2012 Paracetamol: Preparation‚ Purification and Analysis 1.1 Introduction Paracetamol (N- (4- hydroxyphenyl) ethanamide) or acetaminophen is a widely used analgesic (pain reliever) and antipyretic (fever reducer). It is a relatively safe drug though toxicity has been observed with very high doses.1 according to the British Pharmacopeia (BP) 111 paracetamol should contain between 95.0%- 105.0% of the stated product.2 It can be synthesised by reacting 4-aminophenol
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Chapter I Introduction A.) Background of the Study: The Acids‚ bases and salts in the pH range are among the most important chemical compounds used by chemists. For instance‚ hydrochloric‚ phosphoric and citric are acids used to make mineral stain removers‚ toilet bowl cleaners‚ metal cleaners and rust removers. A variety of maintenance chemicals contain these compounds. Alkali maintenance chemicals like degreasers‚ oven cleaners and drain openers contain bases such as Sodium Hydroxide (NaOH)
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ubility * 1 To measure the molar solubility of a sparingly soluble salt in water. * 2 To prepare a calibration curve based on complex ion formation for absorbance enhancement. * 3 To calculate the solubility product constant (Ksp) of a sparingly soluble salt from its molar solubility. * 4 To confirm the common ion effect on the molar solubility of a sparingly soluble salt. Introduction In previous introductory chemistry courses‚ you learned some basic solubility rules that are
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Unknown # 2 Mass of Mohr’s Salt: 0.2040 1. 5mL of 6M acetic acid was measured and transferred into a 100mL volumetric flask with a pipette and diluted to the mark. Concentration = [0.2040(±0.0001)g/100(±0.08)mL]*[(1mol/392.16g)/(1L/1000mL)] = 0.005202(±0.09382%) = 0.005202(±0.000005)mol/L 2. 10mL of the above stock solution was transferred to a 250 mL volumetric flask and diluted to the mark. Concentration = [0.005202(±0.09382%)mol/L]*[10(±0.02)mL/250(±0.12mL)] = 0.00020808(±0
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NH4OH(placed separately into four beakers) was measured using pH meter. And lastly‚ the pH of the solutions was calculated using the obtained values from the procedures. In the third part‚ the percent of acetic acid in vinegar was determined. The buret was rinsed with 0.2M NaOH and was later on filled with the same solution up to its mark of 0.0 ml. 5ml of commercial vinegar‚ 45ml distilled water and two drops of phenolphthalein was placed in the Erlenmeyer flask. The vinegar was titrated with 0
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