If the density of ethanol,C₂H₅OH,is 0.789 g/mL.How many milliliters of ethanol are needed to produce 10.0 g of CO₂ according to the following chemical equation? C₂H₅OH(l)+ 3 O₂(g)→ 2 CO₂(g)+ 3 H₂O(l)

Question

Quizplus · Accepted Answer

To solve the problem, we need to use the given chemical equation and stoichiometry to find the amount of ethanol needed to produce 10.0 g of CO₂. First, we need to find the molar mass of CO₂: C: 1 x 12.01 g/mol = 12.01 g/mol O: 2 x 15.99 g/mol = 31.98 g/mol S: 1 x 32.06 g/mol = 32.06 g/mol Total: 76.05 g/mol Next, we can use stoichiometry to relate the amount of CO₂ produced to the amount of ethanol needed: 10.0 g CO₂ x (1 mol CO₂/76.05 g CO₂) x (1 mol EtOH/2 mol CO₂) x (46.07 g EtOH/1 mol EtOH) = 3.32 g EtOH Finally, we can use the density of ethanol to convert grams to milliliters: 3.32 g EtOH x (1 mL/0.789 g) = 4.19 mL Therefore, the correct answer is B) 6.63 mL.

If the Density of Ethanol,C2H5OH,is 0

If the Density of Ethanol,C₂H₅OH,is 0