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
(You start off with 2.0 mL of ethanol)
volume ethanol that is pure ethanol is 2.00 mL x 0.95 = ? mL.
Then grams ethanol = ? mL x density = grams ethanol.
Convert g ethanol to mols. mols = grams/molar mass = ? mols ethanol.
Using the coefficients in the balanced equation, convert mols ethanol to mols CO2 and mols H2O.
Then g CO2 = mols CO2 x molar mass CO2.
g H2O = mols H2O x molar mass H2O
To find the amount of water and carbon dioxide produced in the reaction, we need to calculate the number of moles of ethanol used and then compare it to the balanced chemical equation.
Step 1: Calculate the number of moles of ethanol used.
We know that the density of ethanol is 0.816 g/mL, and we start with 2.0 mL of ethanol.
Using the density, we can calculate the mass of ethanol:
Mass = volume × density
Mass = 2.0 mL × 0.816 g/mL
Now, let's convert the mass of ethanol to moles using the molar mass of ethanol (C2H6O).
The molar mass of carbon (C) is 12.011 g/mol, the molar mass of hydrogen (H) is 1.00784 g/mol, and the molar mass of oxygen (O) is 15.999 g/mol.
Molar mass of ethanol (C2H6O) = 2 × (molar mass of carbon) + 6 × (molar mass of hydrogen) + (molar mass of oxygen)
Molar mass of ethanol (C2H6O) = 2 × 12.011 g/mol + 6 × 1.00784 g/mol + 15.999 g/mol
Now, divide the mass of ethanol by the molar mass of ethanol to get the number of moles of ethanol used.
Step 2: Compare the moles of ethanol to the balanced chemical equation.
From the balanced equation, we see that for every mole of ethanol, 2 moles of carbon dioxide and 3 moles of water are produced.
So, if we have the moles of ethanol used, we can determine the moles of water and carbon dioxide produced.
Step 3: Calculate the moles of carbon dioxide and water produced.
Using the ratio from the balanced chemical equation, for every 1 mole of ethanol, 2 moles of carbon dioxide and 3 moles of water are produced.
Finally, we multiply the moles of ethanol by the respective ratios to find the moles of carbon dioxide and water.
Let's calculate all the values step-by-step.
To determine the amount of water and carbon dioxide produced in the experiment, we need to calculate the number of moles of ethanol consumed and then use the balanced equation to find the moles of water and carbon dioxide produced.
First, we need to convert the volume of ethanol given (2.0 mL) into grams using the density of ethanol. Since the density of ethanol is 0.816 g/mL, the mass of 2.0 mL of ethanol is:
Mass of ethanol = Density of ethanol × Volume of ethanol
Mass of ethanol = 0.816 g/mL × 2.0 mL
Mass of ethanol = 1.632 grams
Next, we calculate the number of moles of ethanol by dividing the mass by the molar mass of ethanol. The molar mass of ethanol (C2H6O) is:
Molar mass of ethanol = (2 × Atomic mass of carbon) + (6 × Atomic mass of hydrogen) + Atomic mass of oxygen
Molar mass of ethanol = (2 × 12.01 g/mol) + (6 × 1.01 g/mol) + 16.00 g/mol
Molar mass of ethanol = 46.07 g/mol
Number of moles of ethanol = Mass of ethanol / Molar mass of ethanol
Number of moles of ethanol = 1.632 g / 46.07 g/mol
Number of moles of ethanol = 0.0354 moles
Now, using the balanced equation C2H6O + 3O2 → 2CO2 + 3H2O, we can determine the molar ratios between ethanol, water, and carbon dioxide.
From the equation, we know that for every 1 mole of ethanol, 3 moles of water are produced. Therefore,
Number of moles of water produced = Number of moles of ethanol × (3 moles of water / 1 mole of ethanol)
Number of moles of water produced = 0.0354 moles × (3 moles of water / 1 mole of ethanol)
Number of moles of water produced = 0.106 moles
Similarly, we know that for every 1 mole of ethanol, 2 moles of carbon dioxide are produced. Therefore,
Number of moles of carbon dioxide produced = Number of moles of ethanol × (2 moles of carbon dioxide / 1 mole of ethanol)
Number of moles of carbon dioxide produced = 0.0354 moles × (2 moles of carbon dioxide / 1 mole of ethanol)
Number of moles of carbon dioxide produced = 0.0708 moles
Finally, to calculate the mass of water and carbon dioxide produced, we can multiply the number of moles by their respective molar masses.
Mass of water produced = Number of moles of water produced × Molar mass of water
Mass of water produced = 0.106 moles × 18.02 g/mol
Mass of water produced = 1.91 grams
Mass of carbon dioxide produced = Number of moles of carbon dioxide produced × Molar mass of carbon dioxide
Mass of carbon dioxide produced = 0.0708 moles × 44.01 g/mol
Mass of carbon dioxide produced = 3.12 grams
Therefore, in the experiment using 2.0 mL of 95% ethanol by volume, approximately 1.91 grams of water and 3.12 grams of carbon dioxide are produced.