Chemistry - Quantities

Question

For the unbalanced equation shown below, if the reaction of 91.3 grams of C3H6 produces a 81.3% yield, how many grams of CO2 would be produced?

_C3H6 + _O2 → _CO2 + _H2O

Answer 1

Put a 1 in front of C₃H₆. A C balance requires a 3 in front of CO₂. An H balance requires a 3 in front of H₂O. An O balance requires 3(2) + 3 = 9 O or 9/2 O₂ which is ok to have in this context because you usually want these equations to be per 1 mole of fuel.

Now use the stoichiometry to find the ideal yield of CO₂ , then multiply by .813 to find the actual yield:

91.3 g Propene (1 mole/ 42 g P)(3 moles CO₂/1 mole P)(44 g CO₂/mole)(81.3 g CO₂ actual/100g theoretical)

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