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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Title: Stoichiometry of a Precipitation Reaction Purpose: The purpose is to predict the amount of precipitation using stoichiometry. Another purpose is to measure and calculate percentage yield. Procedure: 1. Weigh out 1.0g of CaCl2*2H2O and put it into a 100mL beaker. 2. Add 25mL of distilled water and stir. 3. Using stoichiometry to determine how much Na2CO3 is needed for a full reaction. 4. Weigh the calculated amount and put it in a small paper cup. Add 25mL distilled water and stir
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|| || Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 Convert 1.0g of CaCl2-.2H2O to moles of CaCl2-.2H2O 1.0g x 1 mole CaCl2-.2H2O 147.0 g CaCl2-.2H2O = 0.00680 moles CaCl2-.2H2O The mole ratio is 1:1 Hence if we have 0.00680 moles of CaCl2-.2H2O we will as well need 0.00680 moles of Na-2CO3 Convert moles of Na-2CO3 to grams of Na2CO3 = 0.00680 moles Na-2CO3 x 105.99g Na-2CO3 1
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.6Name: Danielle Hall|Date: 10.15.2012| Exp 9: Stoichiometry of a Precipitation Reaction|Lab Section: | Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 CaCl2.H2O(aq)= m/M =1/147 =0.0068 mol CaCO3(s)=0.0068*1/1 =0.0068 mol CaCO3(s)= CaCO3 (s)= CaCO3 mol *CaCO3 g =0.0068 mol*100.01 g =.68 g Step 4: Mass of weighing dish _0.6___g Mass of weighing dish and Na2CO3 __0.72__g Net mass of the Na2CO3 ___0.12_g Step 6: Mass of filter paper
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Stoichiometry of a Precipitation Reaction Purpose: The purpose of this lab is to calculate the theoretical‚ actual‚ and percent yield of the product from a precipitation reaction. Also‚ to learn concepts of solubility and the formation of a precipitate. Procedure: Weigh out your 1.0g of CaCl2-2H20 and put it into the 100mL beaker‚ Add your 25mL of distilled water and stir to form the calcium chloride solution. Next‚ use stoichiometry to determine how much Na2CO3 and put it into a small
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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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LAB REPORT 7 – STOICHIOMETRY OF A PRECIPITATION REACTION No credit will be given for this lab report if the Data section is not completely filled out. NOTE: This experiment may take several days to complete. OBJECTIVE 1. Predict the amount of product produced in a precipitation reaction using stoichiometry 2. Accurately measure the reactants and products of the reaction 3. Determine the actual and theoretical yield 4. Calculate percent yield PROCEDURE Please complete
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Name: Brian James|Date:3/10/13| Exp 9: Stoichiometry of a Precipitation Reaction|Lab Section: 73426| Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 CaCl2.H2O(aq)= m/M =1/147 =0.0068 mol CaCO3(s)=0.0068*1/1 =0.0068 mol CaCO3(s)= CaCO3 (s)= CaCO3 mol *CaCO3 g =0.0068 mol*100.01 g =.68 g Step 4: Mass of weighing dish _0.6_g Mass of weighing dish and Na2CO3 .72_g Net mass of the Na2CO3 .12_g Step 6: Mass of filter paper
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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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Title: Stoichiometry Reaction Objectives: 1. To decompose sodium hydrogen carbonate (sodium bicarbonate) by heating. 2. To accurately measure the degree of completion of the reaction by analysing the solid sodium carbonate product. 3. To calculate amount of product with given amount of reactant. 4. To determine amount of heat release in the reaction. Results: Part 1: Thermal Decomposition of NaHCO3 Materials Mass (g) Clean and dry test tube 15.1632 Clean test tube + NaHCO3 17.1647
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