#"56.9 g WO"_3"# reacts with excess #"H"_2"# to produce #"W"# and #"H"_2"O"#. What is the percent yield of water if the actual yield is #"10.0 g H"_2"O"#?
#"WO"_3 + "H"_2"# #rarr# #"W+3H"_2"O"#
1 Answer
The percent yield of water is
Explanation:
Start with a balanced equation.
The theoretical yield must be determined. This is done by determining the mass of water expected using stoichiometry. The following represents the steps that must be taken to determine the expected (theoretical) mass of water in this reaction.
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The molar masses of tungsten oxide and water will need to be determined.
Molar Masses
Multiply the subscript of each element by its molar mass, which is its atomic weight on the periodic table in g/mol. Add the results for each substance to get the total.
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Mole Ratios
Determine the mol ratio between
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Multiply the
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Multiply mol
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Multiply mol water by its molar mass.
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Theoretical Yield of Water is
Actual yield is