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Lab 3 Stoichiometry Kaden Miller Grand Canyon University: CHM-113L November 12, 2023
Abstract In chemistry stoichiometry showcases how the law of conservation of matter or mass works. It refers to the relationship and quantities of chemicals involved in a chemical equation. It’s crucial to remember the fundamental principle of thermodynamics, which states that matter cannot be created or destroyed. Stoichiometry explores the connection, between reactants and products in a reaction. For instance when hydrochloric acid reacts with potassium carbonate or sodium carbonate it forms salts, water and carbon dioxide. In this experiment we tested for a relationship between hydrochloric acid and these carbonates.
Introduction We encountered some challenges during the experiment that resulted in a 20% percent error. The equipment used deviated from what was mentioned in the lab manual. Additionally due to time constraints we could only conduct the experiment for an hour. To compensate for missing data we collaborated with peers who conducted experiments using the carbonate. Another example of an acid carbonate reaction is lithium carbonate with hydrochloric acid, which produces lithium chloride. All these examples align, with the law of conservation of mass since matter cannot be created or destroyed. This pertains to the chemical reactions that occur when hydrochloric acid (HCI) is combined separately with sodium carbonate (NaCO3) and potassium carbonate (K2CO3). Understanding this relationship is valuable, for predicting the amount of products obtained from a given reactant. The remaining product should be in the form of a salt. It is important to be familiar with the calculations for yield, percent yield, theoretical yield well as how to balance chemical equations. This laboratory experiment illustrates the stoichiometry between an acid and a carbonate, which react together to produce a salt. When HCI and K2CO3 react potassium chloride (KCI) is formed. Make sure to measure the mass of each piece of equipment. Additionally ensure that you heat and cool the evaporating dish properly. In an evaporating dish 0.5 grams of potassium carbonate was mixed with 2.5mL of 3M HCI solution. The evaporating dish was then placed on a hotplate set at 225 degrees Celsius for 5 minutes in order to dissolve the potassium carbonate completely. During this time keep heating the solution on the hotplate while slightly opening the watch glass covering it. Repeat this step twice while fully covering the dish with the watch glass after each repetition. Once the sample has dried completely you should be left with a salt (KCI). Its weight can be determined using appropriate measurement techniques. Initial data regarding equipment measurements were
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recorded in order to calculate yield, percent yield, theoretical yield and establish an equation, for these reactions. This procedure was then repeated using HCI and sodium carbonate (NaCO3).In the process of a carbonate acid reaction, salts, water and carbon dioxide are produced. When HCI reacts with K2CO3 it forms KCI. Similarly when HCI reacts with NaCO3 it forms NACI. These reactions serve as proof of the connection or quantity, between chemicals in a balanced equation. Data and Analysis Table 1: Mass Data for K2CO3 and HCl Step Descriptions Mass (g) 6 Mass of dish + watch glass 100.165g 7 Mass of dish + watch glass + K2CO3 100.665g 14 Mass of dish + watch glass + KCl 100.962g Table 2: Mass of Data for Na2CO3 and HCl Step Descriptions Mass (g) 6 Mass of dish + watch glass 101.525g 7 Mass of dish + watch glass + Na2CO3 102.027g 14 Mass of dish + watch glass + NaCl 101.835g Table 3: Yeild Caculations for K2CO3 and HCl Step Description Value 2 Mass of K2CO3 (g) 0.50g
3 Mass of KCl (g) 0.80g 4 Theoretical yield of KCl (g) 0.63g 5 Perccent yield of KCl (%) 87.3% Balanced equation: K2CO3 + HCI = H2O + CO2+ KCIMass of K2CO3 using (mass of dish + watch glass and K2CO3) – (mass of dish and watch glass): 100.665g-100.165g = 0.50g Mass of KCI is determined by (mass of dish + watch glass and KCI) – (mass of dish and watch glass):100.962-100.165g=0.80g Theoretical yield of KCI (g) 0.63g Percent yield of KCI= 87.3%(actual yield/theoretical yield x 100%)0.55/0.63 = 0.873 0.8873 x 100= 87.3 0r 87.3% Table 4: Yield Calculations of Na2CO3 and HCl Step Description Value 2 Mass of Na2CO3 (g) 0.50g 3 Mass of NaCl (g) 0.31g 4 Theoretical yield of NaCl (g) 0.23g 5 Percent yield of NaCl (%) 6.7% Balanced equation: NA2CO3 + 2HCI = 2NACI + H2O+ CO2 Mass of NA2CO3 using (mass of dish + watch glass and NA2CO3) – (mass of dish and watch glass):102.027g-101.525g=0.502g Mass of NACI is determined by (mass of dish + watch glass and NACI) – (mass of dish and watch glass):101.835-101.525=0.31g Theoretical yield of NACI (g) 0.23g Percent yield of NACI: 6.74% (actual yield/theoretical yield x 100%)0.015/0.23 = 0.0674
0.0674 X 100 = 6.74% Discussion Random errors can be both unknown and predictable. Such errors may occur when heating the solution of carbonate and acid if the carbonate is not completely dissolved and requires solution. Another possible source of error could be cross contamination when transitioning from NA2CO3 to NACO3. If an excessive amount of HCI solution is added the salt will not react properly. Systematic errors are caused by instruments, methodology, bias or environmental factors. All values obtained or given in this lab report are rounded to two places; however rounding may lead to miscalculations during analysis. This laboratory experiment aimed to demonstrate the relationship between HCI and NA2CO3 well as HCI and KO2CO3. However due to time constraints one hour was allocated for completing the experiment using one acid and one carbonate. Data for the remaining acid carbonate solutions were gathered from fellow classmates experiments. Both carbonates appear as powders while HCI is an acid. Despite having to follow procedures, for both combinations I had hoped to complete both experiments. The laboratory manual provides an example involving lithium carbonate and hydrochloric acid which results in the formation of lithium chloride. Although it may take some time it is possible to conduct three versions of the experiment if given time. Once you are ready to begin writing make sure you have read these instructions thoroughly before deleting them and starting to type. The formatting should remain unchanged except, for the page header located at the top of each page along with the page number.
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Conclusion Stoichiometry demonstrates how the law of conservation of matter or mass can be illustrated. It refers to the proportion or quantity relationship between chemicals in a chemical equation. An example of this is seen in the reaction between hydrochloric acid (HCI) and potassium carbonate (K2CO3) or, betweenhydrochloric acid and sodium carbonate (Na2CO3). This reaction involves heating up a substance and combining it with a liquid to form another substance. The lab manual should be updated with procedures provided for the prelab activities. In actuality conducting this experiment requires a hotplate, dish and watch glass while the lab manual suggests using a cover and Bunsen burner.
References Deo, R. P. (2017). Laboratory manual for general Chemistry I. In Grand Canyon University (Ed.), Laboratory manual for general chemistry I (2nd ed.). Retrieved March 17, 2021, from https://lc.gcumedia.com/chm113l/laboratory-manual-for-general-chemistry-i/v2.1/# chapter/3

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