aliquots of sample solution until you obtain concordant results (titres agreeing within 0.1 mL). 37. Record findings 38. Subtract the initial volume to determine the amount of titrant delivered. Use this‚ the concentration of the titrant‚ and the stoichiometry of the titration reaction to calculate the number of moles of reactant in your analyte solution. 39. Then Calculate the results 40. 1. Calculate the average volume of iodate solution used from your concordant titres. 41. 2. Calculate the moles
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at 20°C is mixed with 30 mL of solution B at 24.0°C and the final temperature reaches 28.0°C? 4. List four dependent variables that are often used for the method of continuous variations. 5. (Skip this question if already covered in another lab) Two thermometers are placed in a sample of water. The first one reads 50.2°C and the second reads 50.9°C. If the second thermometer is placed in a new sample and reads 84.5°C‚ what will the first thermometer read in the same sample? Equipment:
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has reactants and product that has to represent a formulae. The amount of each element‚ number needs to be the same in either side of the equation. (E.g.‚ HCl(aq)+NaHCO3(s) reacts to produce NaCl(aq)+H2O(I)+CO2(g)‚ this is the equation given for 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
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Chem 121L Part I: Introduction Stoichiometry is the study of the quantitative‚ or measurable‚ relationships that exist in chemical formulas and also chemical reactions. In this experiment hydrogen gas will be produced from the reaction of a known mass of magnesium metal with an excess of hydrochloric acid. The theoretical number of moles of hydrogen gas may be calculated using stoichiometry and the balanced chemical equation. The theoretical volume of hydrogen gas may then be determined from
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Hugh Kim Lab Report: Stoichiometry Lab 1. Prelab Part1. 1) Create no waste = The principle that encourages chemists to not create waste at the first place rather than cleaning it up afterwards effectively shifts the chemistry more environmentally conscious‚ as creating no waste would make the experiment efficient; the reactants will be reduced to only the essential ones and the product will be maximized‚ a change that would make the experiment economic. Also‚ if chemists aim to
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wavelength Percentage concentration (methanol: water) Peak H value (height equivalent to a theoretical plate) (mm) 230nm 80:20 Phenol 0.0373 Benzophenone 0.0196 Naphthalene 0.0164 235nm 80:20 Phenol 0.0327 Benzophenone 0.0203 Naphthalene 0.0147 260nm 80:20 Phenol 0.0318 Benzophenone 0.0202 Naphthalene 0.0146 Figure 11: table for the height equivalent of the theoretical plates. It can be observed that the H values or height equivalent to a theoretical plate for phenol at the three wavelengths
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Experiment 9-Dehydration of 2-methylcyclohexanol Name______________________________________________________________________ Lab Partner_________________________________________________________________ Lab Day and Time____________________________________________________________ Report appearance (Typed‚ on time‚ in order‚ presentable‚ complete) 1 2 3 4 5 Abstract 1 2 3 4 5 Introduction 1 2 3 4
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Copper in Silver Nitrate Lab: Making Silver Sabrina Kate S. Carranza – Chemistry Hour 6 I. Purpose: The purpose of this experiment is to distinguish the relationships between reactants and products‚ in addition to expanding on concepts such as single displacement reactions‚ mole ratio values‚ moles to mass‚ theoretical yields‚ limiting reactants‚ excess‚ stoichiometric relationships and percentage errors. II. Hypothesis: /3 -If the copper metal is submerged in the silver nitrate solution
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Lab 3: Bromination of Acetanilide CHEM 2110 Hassan Alsaleh 0525970 Due date :11/02/2015 Q1: To find the limiting reagent we need to find the number of moles of acetanilide‚ and the number of moles of Bromine. Mass of Acetanilide used = 0.67g Molar mass of Acetanilide = 135.16g/mol[1] Number of moles of Acetanilide = (0.67g) / (135.16g/mol) = 0‚005 mols Volume of Bromine = 0.25ml Density of Bromine = 3.103 g/ml[2] Mass of Bromine = (0.25ml) X (3.103g/ml) = 0.78g Molar mass of Bromine
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then that reactants becomes the limiting reactants. Once the limiting reactants will completely be ran out of‚ the reaction is done. So the limiting reactant is the key to start and finish the chemical reaction. B. Procedures and Materials In this Lab‚ we used different procedures and Materials. We had 12.53 gram of copper sulfate pentahydrate and
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