4. Vitamin C, M= 176.12 g/mol, is a compound of composed of carbon, hydrogen, and oxygen. Vitamin C is found in many natural sources especially citrus fruits. When a 1.000-g sample of vitamin C is burned in a combustion apparatus 1.50 g of CO2 and 0.410 g of H2O are produced. What is the empirical formula of Vitamin C? What is the molecular formula of Vitamin C?

I thought you needed to add 0.409 +0.0455 and then subtract them from 1.00? Why did you subtract all of them?

I assume M stands for molar mass.

CxHyOz + O2 --> CO2 + H2O
Convert g CO2 to g C and g H2O to g H.
1.50 g CO2 x (M C/M CO2) = 1.50 x 12/44 = 0.409
0.410 g H2O x (2*1/18) = 0.0455
g O = 1.00 - g C - g H = 1.00 -0.409 - 0.0455 = 0.545 g O
Convert to mols.
mols C = 0.409/12 = 0.0341
mols H = 0.0455/1 = 0.0455
mols O = 0.545/16 = 0.0341
Now you want to find the ratio of C to H to O with no number being less than 1.0. The easy way to start is to divide everything by the smallest number.
C = 0.0341/0.0341 = 1.00
H = 0.0410/0.0341 = 1.33
O = 0.0341/0.0341 = 1.00
These numbers are not small whole numbers so we multiply by integers to obtain, when rounded, small whole numbers.
For example, multiply by 2 to get
C = 0.0341/0.0341 = 1.00 x 2 = 2
H = 0.0455/0.0341 = 1.33 x 2 = 2.66
O = 0.0341/0.0341 = 1.00 x 2 = 2.00
Doesn't work so try 3.
C = 0.0341/0.0341 = 1.00 x 3 = 3.00
H = 0.0455/0.0341 = 1.33 x 3 = 3.99
O = 0.0341/0.0341 = 1.00 x 3 = 3.00
So the empirical formula is C3H4O3 and empirical mass is 88
The molecular formula is always an integer x empirical mass so
empirical mass x integer = 176.12 and round to whole number.
88 x integer = 176.12
integer 176.12/88 = 2.001 which rounds to 2.00 as a whole number so the molecular formula is (C3H4O3)2 = C6H8O6.

Well, it seems like Vitamin C went up in flames! Let's do some chemistry circus tricks to find its empirical and molecular formulas.

First, we need to determine the number of moles of carbon, hydrogen, and oxygen in the given compounds.

For carbon dioxide (CO2), we have 1.50 g. The molar mass of CO2 is 44.01 g/mol, so we can calculate the moles of carbon in CO2.

Moles of carbon = 1.50 g CO2 / 44.01 g/mol CO2 = 0.034 moles of carbon

For water (H2O), we have 0.410 g. The molar mass of H2O is 18.02 g/mol, so we can calculate the moles of hydrogen in H2O.

Moles of hydrogen = 0.410 g H2O / 18.02 g/mol H2O = 0.023 moles of hydrogen

Now, we need to find the moles of oxygen. We can subtract the moles of carbon and hydrogen from the total moles we have.

Moles of oxygen = Moles of substance - Moles of carbon - Moles of hydrogen
= 1.000 g / 176.12 g/mol - 0.034 moles of carbon - 0.023 moles of hydrogen
= 0.568 moles of oxygen

To find the empirical formula, we need to convert these moles into whole number ratios. The simplified ratio would be:

Carbon : Hydrogen : Oxygen = 1 : 2 : 4

So, the empirical formula of Vitamin C is CH2O, which is similar to glucose (just a little citrus twist).

Now, let's flip to the molecular formula! We need to determine the molecular mass of the empirical formula.

Molar mass of CH2O = (12.01 g/mol x 1) + (1.01 g/mol x 2) + (16.00 g/mol x 1) = 30.03 g/mol

To find the molecular formula, we divide the molar mass of Vitamin C by the molar mass of the empirical formula.

Molecular formula = 176.12 g/mol / 30.03 g/mol = 5.87

Hmm, that's not a whole number. So, it seems like the empirical formula is already the molecular formula for Vitamin C!

Voila! The empirical formula and molecular formula of Vitamin C is CH2O.

Remember, Vitamin C is a funny little compound found in citrus fruits, not in a clown's pouch. Keep enjoying those oranges!

To determine the empirical formula of Vitamin C, we need to find the mole ratios between carbon, hydrogen, and oxygen in the compound.

1. Start by calculating the moles of CO2 produced:
Moles of CO2 = mass of CO2 / molar mass of CO2
Moles of CO2 = 1.50 g / 44.01 g/mol = 0.034 moles

2. Next, calculate the moles of H2O produced:
Moles of H2O = mass of H2O / molar mass of H2O
Moles of H2O = 0.410 g / 18.02 g/mol = 0.023 moles

3. Calculate the empirical formula by dividing the moles of each element by the smallest number of moles. The closest whole number ratio will give us the empirical formula.
Carbon: 0.034 moles / 0.023 moles = 1.48 (approximately)
Hydrogen: 0.023 moles / 0.023 moles = 1
Oxygen: 0.034 moles / 0.023 moles = 1.48 (approximately)

The empirical formula is CH1.48O1.48. To simplify, we can round to the nearest whole number ratio, which gives us the empirical formula of CH2O.

To find the molecular formula of Vitamin C, we need to know its molar mass. Given the molar mass of Vitamin C (M = 176.12 g/mol), we can calculate the ratio between the empirical formula mass and the molecular formula mass.

4. Calculate the empirical formula mass:
Empirical formula mass = (mass of C x molar mass of C) + (mass of H x molar mass of H) + (mass of O x molar mass of O)
Empirical formula mass = (1 x 12.01 g/mol) + (2 x 1.01 g/mol) + (1 x 16.00 g/mol)
Empirical formula mass = 12.01 g/mol + 2.02 g/mol + 16.00 g/mol
Empirical formula mass = 30.03 g/mol

5. Find the ratio between the molar mass of the compound (176.12 g/mol) and the empirical formula mass (30.03 g/mol):
Ratio = molar mass of compound / empirical formula mass
Ratio = 176.12 g/mol / 30.03 g/mol
Ratio = 5.86 (approximately)

6. Multiply the subscripts of the empirical formula by the ratio obtained in step 5 to find the molecular formula:
Molecular formula = (C x ratio)H2O
Molecular formula = (1 x 5.86)H2O
Molecular formula = C7H12O6

The empirical formula of Vitamin C is CH2O, and the molecular formula of Vitamin C is C7H12O6.

To determine the empirical formula of Vitamin C, we need to find the ratio of carbon, hydrogen, and oxygen atoms in the compound.

Let's start by calculating the moles of CO2 produced. The molecular weight of CO2 is 44.01 g/mol.

Number of moles of CO2 = mass of CO2 / molecular weight of CO2
Number of moles of CO2 = 1.50 g / 44.01 g/mol

Similarly, let's calculate the moles of H2O produced. The molecular weight of H2O is 18.02 g/mol.

Number of moles of H2O = mass of H2O / molecular weight of H2O
Number of moles of H2O = 0.410 g / 18.02 g/mol

Now, we can use these moles to find the moles of carbon, hydrogen, and oxygen in the compound.

Moles of carbon = 1.50 g of CO2 * (1 mol CO2 / 44.01 g CO2) * (1 mol C / 1 mol CO2)
Moles of hydrogen = 0.410 g of H2O * (1 mol H2O / 18.02 g H2O) * (2 mol H / 1 mol H2O)
Moles of oxygen = 1.50 g of CO2 * (1 mol CO2 / 44.01 g CO2) * (2 mol O / 1 mol CO2) + 0.410 g of H2O * (1 mol H2O / 18.02 g H2O) * (1 mol O / 1 mol H2O)

Now, we have the moles of carbon, hydrogen, and oxygen in the compound. We can simplify these moles by dividing each value by the smallest number to get the empirical formula.

Let's assume the smallest number of moles is for carbon.
Dividing all moles by the moles of carbon:

Moles of carbon (C) = Moles of carbon / Moles of carbon = 1
Moles of hydrogen (H) = Moles of hydrogen / Moles of carbon
Moles of oxygen (O) = Moles of oxygen / Moles of carbon

Now, we need to find the whole number ratio for the empirical formula by multiplying each value by the same factor so that the numbers become whole numbers.

The empirical formula for Vitamin C is the simplest whole number ratio of carbon, hydrogen, and oxygen atoms.

Now, the next step is determining the molecular formula of Vitamin C. The molecular formula represents the actual number of atoms of each element in one molecule of the compound.

To calculate the molecular formula, we need to know the molar mass of Vitamin C. From the given information, the molar mass of Vitamin C is 176.12 g/mol.

Now we can calculate the empirical formula mass by adding the atomic masses for the corresponding elements:

Empirical formula mass = (number of carbon atoms × atomic mass of carbon) + (number of hydrogen atoms × atomic mass of hydrogen) + (number of oxygen atoms × atomic mass of oxygen)

We can then calculate the empirical formula mass of the empirical formula obtained earlier. Let's assume the empirical formula has n carbon atoms, m hydrogen atoms, and k oxygen atoms.

Empirical formula mass = (n × 12.01 g/mol) + (m × 1.01 g/mol) + (k × 16.00 g/mol)

Finally, to determine the molecular formula, we divide the molar mass of Vitamin C by the empirical formula mass calculated earlier:

Molecular formula = Molar mass of Vitamin C / Empirical formula mass

By performing these calculations, you should be able to determine both the empirical and molecular formulas of Vitamin C.