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) + 3O₂(g) → 2CO₂(g) + 3H₂O(l)

Question

Quizplus · Accepted Answer

To calculate the volume of ethanol needed, we need to use stoichiometry to find the number of moles of ethanol required first.

Using the balanced chemical equation: 
1 mol ethanol reacts with 3 mol oxygen to produce 2 mol CO

So, 1 mol ethanol produces 2/3 mol CO

Given mass of CO = 15 g

Molar mass of CO = (12 + 16) g/mol = 28 g/mol

Number of moles of CO = Mass/Molar mass = 15/28 mol

Number of moles of ethanol = (2/3) x (15/28) = 0.357 mol

Now, we can use the density of ethanol to convert moles to volume:

Density of ethanol = 0.789 g/mL

Molar mass of ethanol = (12 + 1 + 16) g/mol = 29 g/mol

Volume of ethanol = (0.357 mol x 29 g/mol) / (0.789 g/mL) = 13.17 mL

Therefore, the answer is B) 9.95 mL, the closest option to 13.17 mL.

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