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Stoichiometry And Chemical Reaction Lab Report

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ADI Lab: Stoichiometry and Chemical Reactions The guiding question of this ADI lab was, “Which balanced equation best represents the thermal decomposition of sodium bicarbonate?” The goal of this lab was to use our knowledge of stoichiometry with the mole ratio to identify the correct chemical equation for the decomposition of sodium bicarbonate. Information that was given going into this investigation was the definition of the law of conservation of mass and the atomic theory which states that no atoms can be created nor destroyed during a chemical reaction. Also the mole ratio which is used to determine how much of a product will be produced in a chemical reaction using the given chemical equation. To conduct the lab, information regarding …show more content…

Before decomposing the sodium bicarbonate, the crucible mass was measured as well as the mass of the crucible with two grams of sodium bicarbonate in it. Two grams of sodium bicarbonate was used because it seemed like a reasonable amount for the size of the crucible and is an easy number to work with in stoichiometry. The sodium bicarbonate was cooked in the crucible for 14 minutes and then the gas was turned off and the crucible was left to cool for 5-10 minutes. Since no information on how long to cook the sodium bicarbonate was given we used our best estimate of how long the substance needed to decompose based off how much was placed in the crucible. Once the crucible was cooled, it was placed on a balance to measure the mass and then subtracted by the mass of the crucible to get the solid product’s mass. Then dimensional analysis was used to find the theoretical yield for the solid substance of each given equation. Starting with 2.0 gram of sodium bicarbonate, the molar ratio from each equation was used to convert from moles of sodium bicarbonate to moles of the solid product in that equation and then molar mass was used to convert the answer back into grams. Once this step was repeated with all four equations the theoretical yield of each was compared with the actual yield found by decomposing the

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In order to begin this experiment, first one must find the balanced chemical equation for the reaction which occurs between the aluminum and copper (II) chloride. This balanced equation being 2Al(s)+3CuCl2 (aq)3Cu(s)+2AlCl3 (aq). After finding this equation, one must use the process of stoichiometry in order to find how many grams of aluminum are needed in order to produce 0.15 grams of copper. In this experiment, the purpose was to produce between 0.1 and 0.2 grams of copper, so one should attempt to produce 0.15 grams of copper seeing as it is the average of those two numbers. The first step in the stoichiometric process which one has to complete is finding how many grams of copper are in one mole of copper.

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Lab 27. Stoichiometry and Chemical Reactions Report In our lab we were asked Which Balanced Chemical Equation Best Represents the Thermal Decomposition of Sodium Bicarbonate. Sodium Bicarbonate is a chemical compound with the formula NaHCO3, also known as baking soda. In the process to answer our guiding question we have to determine how atoms are rearranged during a chemical reaction.

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The actual yield of the reaction was 4.411 grams of copper and was obtained through the experiment

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(0.01 moles of NaOH) x (1 mole Ca(OH)2/ 2 moles of NaOH) = 0.005 moles of Ca(OH)2 Tube 1: (0.0020 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.002 moles of Ca(OH)2 (0.002 moles of Ca(OH)2) x (74.08 grams/mole) = 0.1 grams = theoretical yield Tube 2: (0.0035 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.004 moles of Ca(OH)2 (0.004 moles of Ca(OH)2) x (74.08 grams/mole) = 0.3 grams= theoretical yield Tube 3 (0.0050 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.005 moles of Ca(OH)2 (0.005 moles of Ca(OH)2) x (74.08 grams/mole) = 0.4 grams =theoretical yield Tube

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The data had errors because ratios 1:4, 1:2, and 2:3 all had a neutral PH(7) as seen on graph. This evidence shows that we never had the prefect mole ratio of acetate acid and sodium bicarbonate because we always had left over reactants when tested our ratios. Because our ratios were not perfectly balanced as atomic theory states atoms are not destroyed when when it made the new product and the ratio was not perfectly balanced the was left over

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Materials and Equipment Iron ring and ring stand Crucible and pipe stem triangle Bunsen burner and striker Sodium hydrogen carbonate (baking soda) Scoopula Heat safe gloves Goggles Electronic scale Safety Notes Wear lab goggles in the lab Do not touch crucible without heat safe gloves Allow crucible to cool completely before cleaning out Procedure Mass the crucible. Zero the balance while the crucible is on it and mass 3.00g of baking soda. Place the crucible with baking soda on top of a pipe stem triangle on the ring stand.

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However, the process is both time and temperature dependent, with conversion 90% complete within 75 minutes at 93°C. The reaction proceeds via surface-controlled kinetics; when sodium bicarbonate crystals are heated for a short period of time, very fine needle-shaped crystals of anhydrous sodium carbonate are formed on the sodium bicarbonate surface. Sodium bicarbonate is stable in dry air but slowly decomposes in moist air and should therefore be stored in a well-closed container in a cool, dry place. 5.9. TALC83:

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