If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed…
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Question “If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed…”
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)
Answer
C2H5OH(l) + 3 O2(g) – 2 CO2(g) + 3 H2O(l)
According to stoichiometry
1 mole of ethanol yields 2 moles CO2 (2X44g).
Or, you can say that 1 mole of ethanol will yield 88g CO2.
So 15g can be obtained by 1X15/88 moles = 0.17 Moles of ethanol
We will now convert moles to grams of ethanol
One mole equals 46g of ethanol
So 0.17 moles equals 46 X 0.17g = 7.82 Grams
The following formula can be used to convert grams into mL.
Density = Mass / Volume
so volume = 7.82 grams / 0.789 g / mL = 9.911
mL
Conclusion
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