Stoichiometry of a Precipitation Reaction March 20‚2013 Amber McCollum Introduction Stoichiometry is a branch of chemistry that deals with the quantitative relationships that exist among the reactants and products in chemical reactions To predict the amount of product produced in a precipitation reaction using stoichiometry‚ accurately measure the reactants and products of the reaction‚ determine the actual yield vs. the theoretical yield and to calculate the percent yield. The equation
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Chapter 3: Stoichiometry 3: Stoichiometry 5: Thermochemistry 8: Covalent Bonding and Molecular Structure 15: Chemical Equilibrium 16: Acids and Bases 3.2 Stoichiometry and Compound Formulas 3.1 The Mole and Molar Mass 3.2 Stoichiometry and Compound Formulas 3.3 Stoichiometry and Chemical Reactions 3.4 Stoichiometry and Limiting Reactants 3.5 Chemical Analysis Chapter Summary Chapter Summary Assignment Reference Tools Periodic Table Molarity Calculator Molar Mass Calculator Unit
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CHEM 14 Problem Set 2 Deadline of submission: MHE2 – Feb 7; TFC – Feb 8 SOLVE ALL PROBLEMS. SHOW YOUR SOLUTIONS CLEARLY. 1. Arginine is a semi-essential amino acid that is used to form nitric oxide which in turn plays an important role in the nervous as well as cardiovascular system. It contains C‚ H‚ N and O. Combustion of a 0.75 g pure sample which contains 2.591 x 1021 molecules of the amino acid produced 0.03015 mols of water and 578.59 mL of CO2 at STP. The same sample contains 5.181
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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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In the Stoichiometry Challenge Lab we compared the theoretical results of the reaction between sodium carbonate (Na2CO3) and sulfuric acid (H2SO4) with the actual data we found. I hypothesised that If the mole ratio between Na2SO4 and H2SO4 is 1:1 then when I react 0.5 grams of Na2SO4 (reactant with H2SO4) I should get 0.669 grams of Na2SO4. The actual reaction between .05 grams of Na2CO3 and 5 mL of of H2SO4 produced 0.79g of Na2SO4. When I were testing the reaction‚ I measured out the reactants
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Therefore when I set up my stoichiometry problem I got 3.2 grams NaHCO3 over 1 x 1 mol NaHCO3 over 84.007g NaHCO3 x 1mol Na2CO3 over 2 mol NaHCO3 x 105.987g Na2CO3 x 1 mol Na2CO3. Hence‚ I multiplied 3.2 x 1 x 1 x 105.987 and got 339.1584. Afterwards‚ I divided 339.1584 by 84.007 and got 4.04. Then‚ I divided 4.04 by 2 and got 2.02. In order to get my percent yield I divided 2.02 by 3.2 plus multiplied that by 100 getting 62.8. Now‚ when I had started of the experiment‚ I had
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Experiment 3: Stoichiometry of a Precipitation Reaction Abstract: In this experiment‚ the objective is to use Stoichiometry to predict the amount of product produced in a precipitation reaction. We received working knowledge of how to accurately measure reactants and products of the reaction. We then are able to use the data that we recorded to make assessments of the actual yield opposed to the theoretical yield. When we calculated the percent yield we are able
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Modbury High School SACE Stage 1 Chemistry Topic 5 Mole Concept and Stoichiometry Assignment 5: Volumetric analysis (titrations)‚ stoichiometry SOLUTIONS Note: Write answers neatly and legibly in your exercise book or on pad paper. ALWAYS include a title and name for your work and clearly indicate each answer. 1. a) 23.08 and 23.00 mL are concordant titre values. Average titre = (23.08 + 23.00) = 23.04 mL 2 b) Ca(OH)2
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After concluding the experiment‚ I learned that the products reaction can be created in precise amounts when the masses of the products can be measured to exact standards. Further‚ I learned more about the molarity of aqueous solutions‚ and how that quantity‚ along with the volume of the solution‚ can be manipulated to find the exact number of moles in a given volume. In this case‚ experimenters were given aqueous solutions of NaOH and CaCl2 in known molarities and then had them react with one another
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ordinarily able to measure only the total pressure of a gaseous mixture‚ so if two or more gaseous products are present in the equilibrium mixture‚ the partial pressure of one may need to be inferred from that of the other‚ taking into account the stoichiometry of the
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