Question

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 combustion reaction

Answer 1

The answer is 9.94 ml.

What is density?

• 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,

brainly.com/question/18597444

#SPJ4

The complete question is -

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)