If the density of ethanol,C₂H₅OH,is 0.789 g mL^-1.How many millilitres 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)

Question

Quizplus · Accepted Answer

First, we need to calculate the molar mass of ethanol: 
C2H5OH = (2x12.01 g/mol) + (6x1.01 g/mol) + 16.00 g/mol =46.07 g/mol

Next, we need to use stoichiometry to find the amount of ethanol needed to produce 15.0 g of CO:

15.0 g CO x (1 mol CO/28.01 g) x (1 mol ethanol/2 mol CO) x (46.07 g/ mol) = 9.95 mL ethanol

Therefore, the answer is B) 9.95 mL.

If the Density of Ethanol,C2H5OH,is 0

If the Density of Ethanol,C₂H₅OH,is 0