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!

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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!

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Answer 1 · 2017-04-20T19:27:37

Approx. $600 \cdot g$ $600*g$

Explanation:

We interrogate the stoichiometric equation:

$O {(C_{2} H_{5})}_{2} (l) + 6 O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l)$ $O(C_2H_5)_2(l) + 6O_2(g) rarr 4CO_2(g) + 5H_2O(l)$

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

$Moles of ether$ $"Moles of ether"$ $=$ $=$ $\frac{350 \cdot m L \times 0.713 \cdot g \cdot m L^{- 1}}{74.12 \cdot g \cdot m o l^{- 1}} = 3.37 \cdot m o l .$ $(350*mLxx0.713*g*mL^-1)/(74.12*g*mol^-1)=3.37*mol.$

Given the stoichiometry of the combustion equation, for each mole of ether we combust, $4 \cdot m o l$ $4*mol$ $C O_{2}$ $CO_2$ result.

And thus,

$mass of carbon dioxide = 4 \times 3.37 \cdot m o l \times 44.0 \cdot g \cdot m o l^{- 1} ≅ 600 \cdot g$ $"mass of carbon dioxide"=4xx3.37*molxx44.0*g*mol^-1~=600*g$

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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!

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