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For Review 115 Thus, from the amount of reactants given, the maximum amount of CH 3 0H that can be formed is 6.86 X 10 4 g. This is the theoretical yield. What is the percent yield of CH 3 0H? Actual yield (grams) X Theoretical yield (grams) 3.57 X 104~ 100 = 4 X 100% = 52.0% 6.86 X 10 ~ SEE EXERCISES 3.113 AND 3.114 PROBLEM-SOLVING STRATEGY Solving a Stoichiometry Problem Involving Masses of Reactants and Products 1 ~ Write and balance the equation for the reaction. 2 ~ Convert the known masses of substances to moles. 3 ~ Determine which reactant is limiting. 4 ~ Using the amount of the limiting reactant and the appropriate mole ratios, compute the number of moles of the desired product. 5 ~ Convert from moles to grams, usinq the molar mass. This process is summarized in the diagram below: Balanced chemical equation Masses of known substances Find appropriate mole ratio Convert
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Unformatted text preview: to moles Find limiting reactant Moles desired substance Moles limiting reactant Moles of known substances Use mole ratio to convert Moles of desired product Convert to grams Mass of desired product ~ Key Terms chemical stoichiometry Section 3.2 mass spectrometer average atomic mass Section 3.3 mole Avogadro's number Stoichiometry Deals with the amounts of substances consumed and/or produced in a chemical reaction. We count atoms by measuring the mass of the sample. To relate mass and the number of atoms, the average atomic mass is required. Mole The amount of carbon atoms in exactly 12 g of pure 12C 6.022 X 10 23 units of a substance The mass of one mole of an element = the atomic mass in grams...
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