Consider the balanced equation for the following reaction: 13O2(g) + 2C4H10(g) → 8CO2(g) + 10H2O(l)

Question

Determine the theoretical yield of CO2(g) in grams if the percent yield of CO2(g) is 68.0% and 3.64 moles of CO2(g) forms.

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Answer 1

First, a few things. We know that %_yield = [(Actual Yield) / (Theoretical Yield) ]*100

1. % yield is 68.0%
2. Actual Yield is 3.64 moles
3. Theoretical yield is unknown; we will call this "X"

The first step is to plug in the values you know.

68.0% = ( 3.64mol / X )*100

Dividing each side by 100 gives...

0.680 = 3.64mol / X

Rearrange to isolate X...

0.680X = 3.64 mol

X = 3.64mol/0.680

Therefore, X = 5.35 moles, which is your actual yield.

Now, to convert this to moles, you use the molar mass of CO₂, which is 44.01 g/mol

5.35 moles * (44.01 grams CO₂/ mol CO₂ ) = 235.5 grams of CO₂

Does this make sense?