Consider the reaction of C4H10 with O2 to form CO2 and H2O. If 4.92 g C4H10 is reacted with...
Question:
Consider the reaction of C4H10 with O2 to form CO2 and H2O. If 4.92 g C4H10 is reacted with excess O2 and 10.8 g of CO2 is ultimately isolated, what is the percent yield for the reaction?
Excess Reactant
When a chemical reaction occurs, the reactants become products. As the process moves forward, the relative amounts of reactants become smaller and smaller as the relative amounts of product becomes larger. Once either a reactant is completely used up, the reaction ends. The reactant that is left over is called the excess reactant because it is in excess. No matter how much the excess reactant exists the reaction will not move forward once the limiting reactant is used up. It is like when a car is full of gas but yet it will not start because the air intake is clogged. The gasoline, being an excess reactant, does the car no good as long as there is no oxygen. Since the oxygen is not available the reaction will not proceed forward no matter how much gasoline is in the tank.
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View this answerPercent yield is a calculation to determine the percentage of actual product made in relation to the possible or theoretical amount of product that...
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Calculating Reaction Yield and Percentage Yield from a Limiting Reactant
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How to calculate the theoretical yield? Learn the definition and formula of percent yield. Use the theoretical yield equation to calculate theoretical yield.
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