# Identify the limiting reactant and calculate the mass of a product, given the reaction equation and reactant data. Include: theoretical yield, experimental.

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Identify the limiting reactant and calculate the mass of a product, given the reaction equation and reactant data. Include: theoretical yield, experimental yield Additional KEY Terms Actual yield

Theoretical yield: amounts of product calculated from the limiting reagent. Actual yield: amount produced during the conducted experiment. Percentage yield: ratio of actual to theoretical yield expressed in percentage. actual yield theoretical yield percent yield = x 100

Reactions are influenced by "external" factors which effect the amount of yield produced: 1.Concentration 2.State (s, l, g, aq) 3.Temperature 4.Pressure (of gas reactants) 5.Human error Poor recovery Impurities in reactants Miscalculation A side reaction occurs

5.00 g of KClO 3 is heated and decomposes to yield 1.78 g of O 2. What is the % yield? 3 mole O 2 2 mole KClO 3 1 mole 122.5 g 5.00 g KClO 3 32.0 g O 2 1 mole O 2 = 1.96 g O 2 2 KClO 3  2 KCl + 3 O 2 actual yield theoretical yield percent yield = x 100 1.78 g 1.96 g 90.8 %

How much O 2 would be produced if the percentage yield was 78.5%? Ac. yield Th. yield % yield = x 100 = Ac. yield 1.53 g 1.96 g 78.5 % =

What is the % yield if 58 g H 2 O are produced by combining 60.0 g O 2 and 7.0 g H 2 ? 2 mole H 2 1 mole O 2 32.0 g O 2 60.0 g O 2 2.0 g H 2 1 mole H 2 O 2 (g) + 2 H 2 (g) 2 H 2 O (g) = 7.5 g H 2 H 2 - limiting reactant, O 2 - excess reactant

2 mole H 2 O 2 mole H 2 1 mole H 2 2.0 g H 2 7.0 g H 2 18.0 g 1 mole = 63 g H 2 O produced actual yield theoretical yield percent yield = x 100 58 g 63 g 92 %

CAN YOU / HAVE YOU? Identify the limiting reactant and calculate the mass of a product, given the reaction equation and reactant data. Include: theoretical yield, experimental yield Additional KEY Terms Actual yield

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