Standardize NaOH Average NaOH after 3 trials was 0.6578 M NaOH Moles of HCL Molarity of HCL (average between bottle 1 & 1A) Grams of HCL Grams of Water 4.319g HCL = 4.7181 g H20 Moles of Water in HCL Solution Moles of Water added Moles of ester initially present moles of ester Moles of alcohol initially present Moles of acid present Moles of carboxylic acid present‚ moles of alcohol formed‚ moles of ester disappeared‚ moles of
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sulfur dioxide gas in flask B. moles ethane 10/30 0.33 mol moles SO2 0.33 mol mass SO2 0.33 64 21 g 2 What mass of nitric oxide‚ NO‚ is present in a 2.5 L flask at a pressure of 100 kPa and 0ºC? mole NO 2.5/22.71 0.1101 mol mass NO 0.1101 30 3.3 g 3 Carbon monoxide burns in oxygen according to the equation: 2CO(g) O2(g) → 2CO2(g) Calculate the volume of oxygen required at 25°C and 100 kPa for the combustion of 28 g of carbon monoxide. moles CO 28/28 1 mol
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084×10-1molL-1 =1.492 x 10-3 moles Number of moles of A.S.A can be found by the difference between the mean number of moles of NaOH added for hydrolysis and the mean number of moles of HCl. Avg.vol=sample volumes# of samples Avg. vol = (42.83 + 43.40) 2 = 43.12 mL # of moles of NaOH = Mean vol of NaOH x Molar Conc. Of NaOH = 4.312 x 10-2L ×0.09085molL-1 =3.917 x 10-3 moles # of mol A.S.A = mean # of moles NaOH - mean # moles HCl =
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the number of moles. 3. Find the simplest ratio of moles. Question 1. Mass of elements in g. 2. Number of moles of each element. 3. Simple ratio of elements. Practice problems * A 2.765 g sample of lead oxide was heated in a stream of hydrogen gas and completely converted to elemental lead with a mass of 2.401g. What is the empirical formula of the oxide? Mass of oxygen = 2.765 – 2.401 = 0.364 g Number of moles of oxygen = 0.364/16 = 0.02275 Number of moles of lead = 2.401/20719
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Chemical Reaction – Lab Christian Lecce Mr. Ribarich Wednesday‚ February 20st‚ 2013 Purpose To determine the mass of copper formed when excess aluminum is reacted with a given mass of a copper salt (Copper Chloride dihydrate)‚ and the mole-to-mole ratio between the reactant and the product of a chemical reaction. Apparatus * 150ml beaker * Stirring rod * Ruler * Hotplate * Tweezers * 50ml graduated cylinder Materials * Copper (II) chloride dehydrate
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Processing of Uncertainties | No of moles of Mg in reaction= 0.12524.31= 0.00514 mol (to 3sf)No of moles of Oxygen in reaction= 0.04216.00= 0.00263 mol (to 3sf)No of moles of Mg : No of moles of O= 2:1 ∴ Empirical formula of the compound = Mg2O | Percentage Uncertainty of No of moles of Mg in reaction= 0.0020.125 ×100%= 1.60% (to 3sf)Absolute uncertainty of No of moles of Mg in reaction= 0.00514 × 1.60100= 0.00008 mol (to 5dp)Percentage Uncertainty of No of moles of O in reaction= 100% × 0.0050.042=
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the number of moles of HCl reacted with the NaOH is 0.00216 moles‚ which is less than Gaviscon. The number of moles of NaOH that were added from the burette is 0.00327 moles (1 tablet of Gaviscon). However‚ for Quick-eze‚ the number of moles is 0.00216 moles (1 tablet). This means the average volume of the NaOH have affected the number of moles as the concentration of the sodium hydroxide is 0.1M. This means that if less NaOH was required to neutralise the acid‚ the number of moles of HCl neutralized
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Thermochemistry Lab #2 - Heat of Reaction - Hess’s Law Return The foundation of the study of thermochemistry was laid by the chemist Germain Hess‚ who investigated heat in chemical reactions during the last century. One statement of the law that bears Hess’s name says: The enthalpy change for any reaction depends on the products and reactants and is independent of the pathway or the number of steps between the reactant and product. In this experiment‚ you will measure and compare
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Teresa Meng‚ Niharika Palakodety‚ Victoria Wang‚ and Grace Xiong Mrs. Rhonda Smith Honors Chemistry Period 4 13 May 2012 Redox Reactions Lab Report We wished to investigate the oxidation number of a metal that would form aqueous ions when reacted with an aqueous nitrate salt. For this purpose‚ we chose to investigate the reaction of solid copper metal‚ in the form of a wire‚ with aqueous silver nitrate. Before we began the lab‚ we hypothesized that when silver nitrate‚ AgNO3‚ reacts with
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Compleximetric Determination of Water Hardness Caindec‚ Patricia Ysabel B. Water hardness is a measure of the amount of calcium and magnesium carbonate dissolved as Ca 2+ and Mg 2+ in water. There are no health hazards associated with water hardness‚ however‚ it causes scaling‚ as well as forming of soap suds. Compleximetric titration is one of the best ways of measuring total water hardness using a standard ethylenediaminetetraacetic acid (EDTA) solution. EDTA solution is used as it has the
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