Products Percent Yield. Theoretical Yield Maximum amount of product Calculation Balanced Equation Given mass Molar Mass Mole Ratios.

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Presentation transcript:

Products Percent Yield

Theoretical Yield Maximum amount of product Calculation Balanced Equation Given mass Molar Mass Mole Ratios

Actual Yield Amount of product from an experiment. What are these?

Why are they not the same? Reactants and product stick to containers Competing reactions Other ideas?

Percent Yield

LiOH + HBr  LiBr + H 2 O If you start with 10.0 grams of lithium hydroxide, how many grams of lithium bromide will be produced? Find percent yield if an experiment yielded 35.0 grams of lithium bromide.

LiOH + HBr  LiBr + H 2 O 10 g LiOH 1 mol LiOH 1 mol LiBr 87 g LiBr = 36.3 g LiBr 24 g LiOH 1 mol LiOH 1 mol LiBr Given 10 g mass-to-mole mole mole-to-mass unknown ratio mass

C 2 H O 2  2 CO H 2 O If you start with 45 grams of ethylene (C 2 H 4 ), how many grams of carbon dioxide will be produced? Find percent yield if an experiment yielded grams of carbon dioxide.

C 2 H O 2  2 CO H 2 O 45 g C 2 H 2 1 mol C 2 H 2 2 mol CO 2 44 g CO 2 = 141 g CO 2 28 g C 2 H 2 1 mol C 2 H 2 1 mol CO 2 Given 45 g mass-to-mole mole mole-to-mass unknown ratio mass

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