chem

One method for reclaiming silver metal from silver chloride results in a 94.6%
yield. Calculate the actual mass of silver that can be produced in this reaction
if 100.0 g of silver chloride is converted to silver metal.
2AgCl(s) y 2Ag(s) . Cl2(g)

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  1. Write the equation which you have BUT you have omitted the yield sign and and + signs. No way to know the difference between reactants and products.
    Convert 100.0 g AgCl to mols.
    Using the coefficients in the balanced equation, convert mols AgCl to mols Ag.
    Convert mols Ag to grams Ag by grams = mols x molar mass.
    Substitute in the earlier problem for the percent yield and solve for the actual amount. Post your work if you get stuck.

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  2. hgj

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  3. 2AgCl(s) y 2Ag(s) 1 Cl2(g)

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  4. 100.0 g AgCl * 1 mol AgCl/143.5 g AgCl * 2 mol Ag/2 mol AgCl * 108 g Ag/1 mol = 75.3 g Ag, mass of Ag(s) reclaimed = 0.946 * 75.3 g Ag = 71.2 g Ag. Hope it helps :)

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