What is the mass (in grams) of carbon dioxide generated if 361 mL of ethanol is burnt in excess oxygen? Answer to 0 decimal points.

To answer this question, we need to know the balanced chemical equation for the combustion of ethanol (C2H5OH) in oxygen, which is:

C2H5OH + 3O2 -> 2CO2 + 3H2O

From this equation, we can see that 1 mole of ethanol produces 2 moles of carbon dioxide.

We also need to know the density of ethanol, which is 0.789 g/mL, and the molar mass of ethanol, which is 46.07 g/mol. The molar mass of carbon dioxide (CO2) is 44.01 g/mol.

Step 1: Convert the volume of ethanol to mass using its density. Mass = Volume x Density Mass = 361 mL x 0.789 g/mL = 284.7 g

Step 2: Convert the mass of ethanol to moles using its molar mass. Moles = Mass / Molar mass Moles = 284.7 g / 46.07 g/mol = 6.18 mol

Step 3: Use the stoichiometry of the reaction to find the moles of carbon dioxide produced. From the balanced equation, 1 mole of ethanol produces 2 moles of CO2. So, 6.18 moles of ethanol will produce 2 x 6.18 = 12.36 moles of CO2.

Step 4: Convert the moles of CO2 to mass using its molar mass. Mass = Moles x Molar mass Mass = 12.36 mol x 44.01 g/mol = 543.8 g

So, the mass of carbon dioxide generated if 361 mL of ethanol is burnt in excess oxygen is approximately 544 grams (rounded to 0 decimal points).