final lab - was measured with a mass of .46 grams AgCl....

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Olivia Downs December 1, 2010 Section 9 Can you prepare 0.5 g of product? In this experiment, we were asked to prepare 0.5 grams of either Cu metal or AgCl, balance the chemical equation, and determine the type of reaction it was. The investigation began by balancing the chemical equation for our given product. Our group was assigned Silver Chloride. Next, calculations were then done for each reactant to see how many milliliters of silver nitrate and calcium chloride were needed from 0.5 grams of silver chloride product. The two amounts of the reactants, 3.4 mL CaCl2 and 6.9 mL AgNO3, were measured onto a filter pack to form the product. A splint test was then performed. The product was put into an oven to heat until dry for accurate measurements. Once the product was dry, it
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Unformatted text preview: was measured with a mass of .46 grams AgCl. This mass was then inserted in the percent yield equation: (Actual Yield/ Theoretical Yield) X 100%. The experiment was done in this manner because We can argue that 0.5 grams of a product can be prepared because our group managed to prepare an actual yield of .46 grams of silver chloride. This was our balanced chemical equation: CaCl2(aq) + 2AgNO3(aq) -> Ca(NO3)2(aq) + 2AgCl(s). This equation is a redox reaction. The total percent yield was 92%. This information supports the fact that this amount of product can be made successfully. Other lab groups has successful results, but with the product of copper....
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This note was uploaded on 11/03/2011 for the course CHM 1045 taught by Professor Jackson during the Fall '10 term at Tallahassee Community College.

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