# How many grams of CO2 would be produced if 350.0 mL of diethyl ether were combusted in an unlimited amount of oxygen ? Density of diethyl ether is 0.713g/mL. C4H10O + O2 ---> H2O + CO2 Thanks for all your content!

Apr 20, 2017

Approx. $600 \cdot g$

#### Explanation:

We interrogate the stoichiometric equation:

$O {\left({C}_{2} {H}_{5}\right)}_{2} \left(l\right) + 6 {O}_{2} \left(g\right) \rightarrow 4 C {O}_{2} \left(g\right) + 5 {H}_{2} O \left(l\right)$

Is this thing balanced? It is your problem not mine!

$\text{Moles of ether}$ $=$ $\frac{350 \cdot m L \times 0.713 \cdot g \cdot m {L}^{-} 1}{74.12 \cdot g \cdot m o {l}^{-} 1} = 3.37 \cdot m o l .$

Given the stoichiometry of the combustion equation, for each mole of ether we combust, $4 \cdot m o l$ $C {O}_{2}$ result.

And thus,

$\text{mass of carbon dioxide} = 4 \times 3.37 \cdot m o l \times 44.0 \cdot g \cdot m o {l}^{-} 1 \cong 600 \cdot g$