Assuming the solution you used was 95% ethanol by volume and that the density of ethanol is 0.816g/mL, how much water and carbon dioxide are produced in the experiment?

Equation: C2H6O+3O2-->2CO2+3H2O

It really would have been nice if you told us how much ethanol (I presume that is number of mL) but you didn't type that in. Can't work the problem without proper information.

To determine how much water and carbon dioxide are produced in the experiment, we need to use the given information and use the stoichiometry of the balanced equation.

The equation provided is a balanced equation for the combustion of ethanol (C2H6O) in the presence of oxygen (O2). According to the equation, one molecule of ethanol reacts with three molecules of oxygen to produce two molecules of carbon dioxide (CO2) and three molecules of water (H2O).

Given that the solution used is 95% ethanol by volume, we can assume that we have 95 mL of ethanol. To calculate the mass of ethanol, we multiply its volume by its density:

Mass of ethanol = 95 mL × 0.816 g/mL = 77.52 g

To determine the amount of ethanol in moles, we divide the mass of ethanol by its molar mass, which is approximately 46.07 g/mol:

Moles of ethanol = 77.52 g ÷ 46.07 g/mol ≈ 1.685 mol

From the balanced equation, we can see that two moles of carbon dioxide and three moles of water are produced for every one mole of ethanol reacted.

Therefore, the moles of carbon dioxide produced would be:

Moles of carbon dioxide = 2 × 1.685 mol ≈ 3.37 mol

Similarly, the moles of water produced would be:

Moles of water = 3 × 1.685 mol ≈ 5.055 mol

To convert the moles of carbon dioxide and water into their respective masses, we need to multiply by their molar masses. The molar mass of carbon dioxide (CO2) is about 44.01 g/mol, and the molar mass of water (H2O) is approximately 18.02 g/mol.

Mass of carbon dioxide = 3.37 mol × 44.01 g/mol ≈ 148.14 g

Mass of water = 5.055 mol × 18.02 g/mol ≈ 91.09 g

Therefore, approximately 148.14 g of carbon dioxide and 91.09 g of water are produced in the experiment.