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Scan_Doc0022 - to moles Find limiting reactant Moles...

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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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