Kinetics of the Decomposition of Hydrogen Peroxide Lab Introduction: In this week’s lab experiment‚ the rate of decomposition of hydrogen peroxide forming oxygen gas will be observed and studied. Since the rate of a chemical reaction is dependent on two things; the concentrations of the reactants and the temperature at which the process is performed‚ the rate can be measured at which a reactant disappears or at which a product appears. When measuring the rate‚ the rate law will be applied. The
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by Georg Wittig in 1954‚ the Wittig reaction is a robust organic synthesis method for preparing stereospecific alkenes. In general‚ Wittig reactions involve an aldehyde or ketone and a Wittig reagent (triphenylphosphonium ylide) and result in the formation of an alkene product and triphenylphosphine oxide (side product). Stereospecific alkene products can be synthesized by adjusting the reaction reagents and conditions. In the 60 years since the Wittig reaction was discovered‚ many articles have
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three reactions that occurred in the test tubes where you combined potassium iodide‚ KI‚ and hydrogen peroxide‚ H2O2 (in part 1) of the experiment? (Give a detailed explanation of any observations that you made‚ i.e.‚ what made the colour change‚ what reactions happened?) ANSWER: 2. Use the information below to develop the necessary calculations for the rate of reaction from the solutions in part B of the experiment • Calculate the initial molarity
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The purpose of this experiment was to synthesize triphenylmethanol from a Grignard reagent. The Grignard reaction technique was used in this synthesis but due to the fact that it is such a strong nucleophile and base‚ it was important to prevent water from interfering with the Grignard reaction. Purity of the product was determined by measuring the melting point. Reagent Table: Structure Name Molecular formula Molar mass Density Melting point Boiling Point Diethyl ether C4H10O
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this lab). This help us view the study of Law of Conservation of Mass‚ when either side of equation is equally balanced. The calculation for formula mass helps determine if you need to convert grams to a particular substance to moles‚ from a product. Moles are numbers that are in front of formulae. E.g.‚ 6NaCl‚ 6 is the equation for this formula. A mole would help you balance a skeleton equation‚ and also allows you to calculate how many moles are needed to take part in a chemical reaction. In the
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eventually falls in the liquid with a constant speed of 6.0 cm s . k www.studyguide.pk www.studyguide.pk www.studyguide. (i) For this sphere travelling at constant speed‚ calculate k www.studyguide.pk www.studyguide.pk www.studyguide. 1. its kinetic energy‚ k www.studyguide.pk www.studyguide.pk www.studyguide. k www.studyguide.pk www.studyguide.pk www.studyguide. k www.studyguide.pk www.studyguide.pk www.studyguide. k www.studyguide.pk www.studyguide.pk
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Organic Chemistry II Lab Diels Alder Reaction Purpose: In this experiment a Diels-Alder reaction was used to form the products. Cyclopentadiene and maleic anhydride were reacted together to form cis-Norbornene-5‚6-endo-dicarboxylic anhydride. 7-oxabicyclo{2.2.1}hept-5-ene-2‚3-dicarboxylic anhydride was also produced through a Diels-Alder reaction with the combination of furan and maleic anhydride. Equation: Procedure: Part 1 In a flask equipped with
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INTRODUCTION The lab introduced the relationship between reactants and products‚ and sought to discover which ratio of an acid and base reaction produced the most amount of carbon dioxide gas (CO2) without leaving leftover reactants. 5 varying amounts of bases were added to a constant amount of acid (10 ml) to better understand which ratio was the most efficient. RESULTS Data collected from the lab suggests that the ratio of acid to base that produced the most carbon dioxide gas (CO2) was 1:0.5
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ab: Observing a Chemical Reaction Name: Deja Eason Period: 5th Period Partners: Melingh Patterson‚ Tori Millens Date Performed: 9/2/11 Teacher: Mrs. Medina Abstract: This experiment was all about observing a chemical reaction. During the experiment‚ we made observations and possible explanations on why Copper(II)Chloride Dehydrate and Aluminum foil created a chemical reaction. The observations were made by using Copper Chloride‚ Aluminum foil‚ and Distilled water. Before the Aluminum
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Qualitative Observations of Double Displacement Reactions Lab Table 1.0 Qualitative Observation of Products Formed |Balanced Chemical Equations |Qualitative Observations | |BaCl2 (aq) + 2NaOH (aq)( BaOH2(aq) + 2NaCl(s) |An aqueous solution formed | | |Precipitate
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