Date Performed: January 10 & 15‚ 2013 Spectrophotometric Determination of the Equilibrium Constant of a Reaction R.J.V. Ortega and J.C.V. Gatdula Institute of Chemistry‚ College of Science University of the Philippines‚ Diliman‚ Quezon City‚ Philippines Received January 22‚ 2013 ------------------------------------------------- ------------------------------------------------- ------------------------------------------------- ABSTRACT -------------------------------------------------
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three experiments are to determine the heat capacity of a calorimeter and with that data‚ confirm Hess’s Law and observe enthalpy changes within reactions. By measuring the change in temperature that occurs with the interaction of two different reactants‚ we were able to determine both the calorimeter constant and the change in enthalpy of a given reaction. The results were rather mixed‚ as some numbers more closely resembled the theoretical values than others did. Introduction The first experiment
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reaction‚ as well as the risk of undesirable products due to the presence of water. The components of the two stage reaction were as follows: An organic phase containing the alkene and CHCl2; and an aqueous phase containing the base OH –. Since the reactants‚ CHCl2 and OH – would separate into different phases‚ benzyltriethylammonium chloride was added as a phase-transfer catalyst. Because the benzyltriethylammonium chloride has both hydrophilic and hydrophobic properties‚ it could cross the phase boundary
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Chemistry June Exam Notes Quantities in Chemical Reactions Molecular and formula mass o The mass of one unit of a compound (a molecule or a formula unit) o The sum of the mass of all the atoms in a compound o With knowledge of the mass of each individual atom‚ the percentage composition by mass can be determined The Mole (mol) o A counting unit‚ one mole refers to 6.02 x 1023 particles of any given substance o Known as Avogadro’s Constant and given the symbol NA Molar Mass o The
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water is produced. In double mixed aldo condensation of acetone and benzaldehyde‚ the α-hydrogen’s on both sides of the acetone deprotonates and a nucleophilic enolate anion arises as a result. In an aldol condensation many products are formed there reactant are more than one thus the aldehyde reacts with itself to yield a product. The product formed in an aldol condensation contains and adehydes and an alcohol. Claisen-Schmidt condensation is a crossed aldol condensation that involves an aromatic aldehydes
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from sunlight. Photosynthesis involves three ‘ingredients’ or reactants‚ carbon dioxide‚ water‚ and light energy (sunlight). Carbon dioxide and sunlight come in through a leaf’s stomata which are tiny holes‚ and water is absorbed through their roots. When all of these reactants are combined in a plant’s chloroplasts‚ glucose (a type of energy) and oxygen are produced. In the experiment a limiting factor is the light intensity. Limiting factors are any factors in an experiment which may limit the results
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COE CHEMONE Reviewer for CHEMONE Finals Rules for Counting Significant Figures 1. Nonzero integers. Nonzero integers always count as significant figures. 2. Zeros. There are three classes of zeros: a. Leading zeros are zeros that precede all the nonzero digits. These do not count as significant figures. In the number 0.0025‚ the three zeros simply indicate the position of the decimal point. This number has only two significant figures. Note that the number 1.00 _ 102 above is written in exponential
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Questions Experiment 1 Calibration of the calorimeter: 1. Give the net ionic thermochemical equation of the reaction used to calibrate the calorimeter. a. Is the reaction endothermic or exothermic? b. Which is the limiting reactant? c. How much (in moles) limiting reactant was used? d. How much heat was generated (or absorbed) by the reaction? 2. Relate the sign of the ΔT to the ΔH of the reaction used for calibration. 3. What is the heat capacity of the calorimeter? Relate its sign to
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calorimeter. The heat capacity (Ccal) of each calorimeter was calculated using the formula‚ C_cal=(-〖∆H〗_rxn^o n_LR)/∆T [1] where ∆Horxn is the total heat absorbed or evolved for every mole of reaction and nLR is the number of moles of the limiting reactant. The ∆Horxn used was -55.8kJ per mole of water while the nLR was 0.005 mole. Table 1. Average Ccal from recorded ∆T values. Trial ∆T‚ (oC) Ccal‚ (J) Ave Ccal‚ (J) 1 1 2.2 126.82 202.91 2 1.0 279.00 2 1 3.0 93.00 108.50 2 2.3 124.00
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Experiment 3: Stoichiometry of a Precipitation Reaction Abstract: In this experiment the objectives were to try and predict the amount of product that was produced in the precipitation reaction of calcium carbonate by using stoichiometry. Then learn how to figure out the actual yield‚ theoretical yield and percent yield of the experiment. Experiment and Observation: The first step in the experiment was to weigh 1g of CaCl2 +2 H2O‚ then pour it into the 100mL
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