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)
C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l)
As per stoichiometry of the equation
1 mole of ethanol will give 2 moles of CO2 (2X44g)
Or we can say 88g of CO2 will be obtained from 1 mole of ethanol
So 15g will be obtained from 1X15 / 88 moles = 0.17 moles of ethanol
Now we will convert moles of ethanol to grams
1 mole is equal to 46g of ethanol
so 0.17 moles will be equal to 46 X 0.17 g = 7.82 grams
we can convert the grams to mL by followng formula
Density = mass / volume
so volume = 7.82 grams / 0.789 g / mL = 9.911 mL
If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed...
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The density of ethanol is 0.789 g/mL. What is the density in units of kg/m3?