# How to calculate the number of moles of CO2 produced?

May 31, 2017

We work out the molar equivalence of each reagent.....but we strikes a problem..........

#### Explanation:

${C}_{3} {H}_{6} \left(g\right) + \frac{9}{2} {O}_{2} \left(g\right) \rightarrow 3 C {O}_{2} \left(g\right) + 3 {H}_{2} O \left(g\right)$

The arithmetic is a bit easier if we use this half-integral coefficient. Is it balanced? Don't trust my arithmetic.

$\text{Moles of propylene} = \frac{25 \cdot g}{42.08 \cdot g \cdot m o {l}^{-} 1} = 0.594 \cdot m o l$.

$\text{Moles of dioxygen} = \frac{80 \cdot g}{32.00 \cdot g \cdot m o {l}^{-} 1} = 2.50 \cdot m o l$.

And thus there is INSUFFICIENT dioxygen gas for complete combustion. We cannot assess the moles of carbon dioxide produced. Carbon, as particulate soot, and carbon monoxide, as the products of INCOMPLETE combustion, would occur in the product mix.

Since we have no idea of the product mix, the question is a bit of a $\text{non-sequitir}$, and should not have been asked. A mass of $86 \cdot g$ of dioxygen should have been supplied.