Lab 1: Synthesis of Aspirin Introduction: The purpose of this lab was to demonstrate the ability to easily alter the molecular structure of a compound to greatly increase its utility. In this case‚ an acetyl group was added to salicylic acid‚ a naturally occurring compound with significant pharmaceutical value. Without the addition of the acetyl group‚ salicylic acid is an irritant to the gastro-intestinal (GI) tract. Once the acetyl group is added via a simple reaction‚ acetylsalicylic
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all of the CaCO3 and then titrating the remaining unreacted HCl with NaOH solution to determine the amount of acid which did not react with the calcium carbonate. The difference between the moles of the acid (HCl) initially added and the moles of HCl left unreacted after the reaction‚ is equal to the moles of HCl that did react with CaCO3. The reaction used to determine the amount of unreacted acid by titration is given below. This type of analysis is generally referred to as a back-titration
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150.0 mL of a 3.50 M solution? (Assume that the molecular weight of CaBr2 is 200.618 g/mol) 105 g Nitrous oxide (N2O)‚ or laughing gas‚ is commonly used as an anesthetic in dentistry and surgery. How many moles are present in 8.4 liters of nitrous oxide at STP? 0.375 moles How many moles of gas molecules will be present in 5000 L of air at STP? 223.2 mol How many molecules are in 1 mol of sucrose (C12H22O11)? | |6.02 × 1023 molecules | | |What is the empirical
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Laboratory report Aluminum Copper Alloy MSCI 300 – Thermodynamics of Materials Alexandre de Freitas Silveira Eau Claire December 18th‚ 2012. Abstract: At this experiment‚ the composition of an alloy of Aluminum Copper was analyzed via X-Ray Fluorescence. From this‚ it was possible to construct a phase diagram a make some predictions about the possible phases presents at considering the 3 samples used in this experiment‚ the samples prepared at this experiment the sample as delivered
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Unit 16 Study Guide 1. Which of the following statements concerning equilibrium is not true? A) A system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. B) Equilibrium in molecular systems is dynamic‚ with two opposing processes balancing one another. C) The value of the equilibrium constant for a given reaction mixture is the same regardless of the direction from which equilibrium is attained. D) A system moves spontaneously
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Lecture 12 Chapter 6 6.1 Thermochemistry: Energy & units (p.227) From observation we know‚ that - some chemical reactions begin as soon as the reactants come into contact with each other (precipitation reactions) - some reactions are slow or even so slow at room temperature that even lifetime is not enough to observe a measurable change (rusting of iron‚ tarnishing silver) Also‚ almost all chemical reactions involve exchange of heat (or energy): in combustion reactions
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OH- ions in this way releases energy. In this practical‚ the enthalpy changes accompanying different neutralization reactions will be measured. It is because the number of moles of water formed varies according to the acid and alkali used‚ it is the convention to measure enthalpy change of neutralization in kJ mol-1 when 1 mole of water is formed. We will use a simple calorimeter to determine the enthalpy change of neutralization for the pairs of acid and base given. Apparatus and Materials: 1
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different substances (HCl and NH4OH) were inserted into the two ends of the glass tube. The substance with the lighter molecular weight value (NH 4OH‚ M = 35.0459 g/mole) diffused at a faster rate (dAve = 25.8cm)‚ resulting in the formation of a white ring around the glass closer to the side of the heavier substance (HCl‚ M = 36.4611 g/mole; dAve = 10.8 cm). The agar-water gel set up was composed of a petri dish of agar-water gel containing three wells. Drops of potassium permanganate (KMnO4)‚ potassium
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Using the Iodine clock method to find the order of a reaction Introduction When peroxodisulfate (VI) ions and iodide ions react together in solution they form sulfate (VI) ions and iodide. This reaction is shown below: S2O82-aq+ 2I-aq SO42-aq+ I2(aq) The reactants and the sulfate (VI) ions are colourless however the Iodine is a yellow/brown colour. This allows you to measure the progress of the reaction through the colour change when the iodine is produced. In order to determine the order of
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vinegar to produce carbon dioxide‚ water‚ and calcium acetate as represented by the equation: CaCO3 + 2HC2H3O2 CO2 + H2O + Ca(C2H3O2)2. The calcium carbonate reacts with the acetic acid in a 1:2 ratio. Therefore‚ for every one mole of calcium carbonate that reacts‚ 2 moles of acetic acid have reacted as well. Materials: 1. Broken eggshells 2. 2 125 mL flasks 3. Stirring rod 4. 25 mL vinegar 5. Filter paper 6. Funnel 7. Electronic balance 8. Paper towels 9. Weighing paper Procedure: 1
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