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2 years ago

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The density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 via a combust

ion reaction

1 answer:

bearhunter [10]2 years ago

5 0

<u>The answer is </u><u>9.94 ml.</u>

<h3>What is density?</h3>

Density is a word we use to describe how much space an object or substance takes up (its volume) in relation to the amount of matter in that object or substance (its mass).
Another way to put it is that density is the amount of mass per unit of volume. If an object is heavy and compact, it has a high density.

Given,

The density of ethanol, C2H5OH = 0.789 g/mL

$n (CO_{2} ) = \frac{m}{M} = \frac{15G}{44 g/mol} } = 0.341 mol;$

$n ( C_{2} H_{2} OH) = \frac{n (CO_{2}) }{2} = \frac{0.341}{2} = 0.1705 mol;$

$m (C_{2} H_{2} OH) = 0.1705 mol * 46 g/ mol$ = 7.843 g

$V (C_{2} H_{2} OH ) = \frac{7.843}{0.789} = 9.94 ml.$

Therefore, the answer is 9.94 ml

Learn more about density of ethanol,

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<u>The complete question is -</u>

If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation?

C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)

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