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Example One If 100g of CO reacts with an excess of H2 to form 75g CH3 OH, what is the percent yield of the reaction? The balanced equation is CO + 2 H2 = CH3 OH. First, determine the theoretical yield. You have mass of the reactant CO, so you need to change this to moles of CO. Use the mole ratio and then determine the theoretical amount of CH3 OH that will be made. Mass of CO (use the molar mass equivalent here) = moles CO (use the mole ratio here to change moles to moles) = moles CH3 OH (use the molar mass equivalent here) = mass CH3 OH= percent yield. 100g CO x 1 mole CO / 28g CO = 3.6 moles CO 3.6 moles CO x 1 mole CH3 OH / 1 mole CO = 3.6 moles CH3 OH 3.6 moles CH3 OH x 32g CH3 OH / 1 mole CH3 OH = 115.2 g CH3 OH. This is the theoretical yield. Percent yield = actual yield/theoretical yield x 100% Percent yield = 75g CH3 OH / 115.2 g CH3 OH x 100% = 65% The percent yield for example one is determined by solving this equation. Percent Yield Example One
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