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Stoichiometric Calculations<br />The coefficients in the balanced equation give the ratio of moles of reactants and products<br />
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Stoichiometric Calculations<br /> From the mass of Substance A you can use the ratio of the coefficients of A and B to calculate the mass of Substance B formed (if it’s a product) or used (if it’s a reactant)<br />
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Stoichiometric Calculations<br />C6H12O6 + 6 O2 6 CO2 + 6 H2O<br /> Starting with 1.00 g of C6H12O6… <br /> we calculate the moles of C6H12O6…<br /> use the coefficients to find the moles of H2O…<br /> and then turn the moles of water to grams<br />
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Sample #1<br />CH4 +2O22H2O + CO2<br />How many moles of CH4 are needed to make 13 moles of water?<br />
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Sample #2<br />CH4 +2O22H2O + CO2<br />How many moles of water are made from 10g of Oxygen?<br />
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Sample #3<br />CH4 +2O22H2O + CO2<br />How many grams of water are produced from 100 moles of CH4?<br />
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Sample #4<br />CH4 +2O22H2O + CO2<br />How many grams of Oxygen are needed in order to produce 200 g of carbon dioxide?<br />
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Limiting Reactants<br /> The limiting reactant is the reactant present in the smallest stoichiometric amount<br />
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Limiting Reactants<br />The limiting reactant is the reactant present in the smallest stoichiometric amount<br />In other words, it’s the reactant you’ll run out of first (in this case, the H2)<br />
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Limiting Reactants<br /> In the example below, the O2 would be the excess reagent<br />
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Theoretical Yield<br />The theoretical yield is the amount of product that can be made<br />In other words it’s the amount of product possible as calculated through the stoichiometry problem<br />This is different from the actual yield, the amount one actually produces and measures<br />
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Percent Yield<br />Actual Yield<br />Theoretical Yield<br />Percent Yield = x 100<br /> A comparison of the amount actually obtained to the amount it was possible to make<br />
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