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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.
- Fall '10