what is the molecular formula of a compound that is 54.5% C, 9.09% H, and 36.4% O. with a molecular weight of 176g/mol.

A)C8H16O4
B)C4H8O2
C)C7H12O5
D)C9H18O3

Assume you have 100 g of the substance, then you have 54.5g of C, etc.

Moles C= 54.5/12=4.54 mol
Moles H=
Moles O=

Then, divide all these moles each by the lowest in the table above. That will give you the empirical formula, example
where the mole mass is 220
Moles C= 3.2
Moles H= 6.4
Moles O= 19
divide by lowest, 3.2
Moles C= 1
Moles H= 2
Moles O= 6
CH2O6 empirical formula, emperical molmass is 12+2+6*16= 110 Divide this into the given mol mass (220/110=2), so multiply the atom ratios by this: mol formula C2H4O12

So finish the problem, if you get stuck, repost

how do u get the empirical molmass ?? nowher in the sample ugave s thre a 12 2 a 6 and why multiply by 16??

The empirial mass is the sum of the atoms atomic mass in the empirical formula

CH2O6 C is 12, H is 1, but there are two of them, and there are 6 O or 6*16. Sum is the empirical mass.

kmno4

kmno4 + c3h8o3

To calculate the empirical molar mass, you need to consider the atomic masses of the elements in the empirical formula. In this case, the empirical formula is CH2O6.

The atomic mass of carbon (C) is 12, the atomic mass of hydrogen (H) is 1, and the atomic mass of oxygen (O) is 16.

In the empirical formula CH2O6, there is 1 carbon atom (12), 2 hydrogen atoms (2 * 1 = 2), and 6 oxygen atoms (6 * 16 = 96).

Adding up the masses of each element: 12 + 2 + 96 = 110.

Therefore, the empirical molar mass of the compound is 110 g/mol.

Now, let's use this information to find the molecular formula of the compound.

The given molecular weight of the compound is 176 g/mol.

Divide the molecular weight by the empirical molar mass: 176 / 110 = 1.6.

Multiply the subscripts in the empirical formula by this ratio:

Carbon (C): 1 * 1.6 = 1.6
Hydrogen (H): 2 * 1.6 = 3.2
Oxygen (O): 6 * 1.6 = 9.6

Round these numbers to the nearest whole number to get the subscripts in the molecular formula:

C1.6H3.2O9.6

Converting the decimal numbers to whole numbers:

C2H4O12

The molecular formula of the compound is C2H4O12.

Comparing this with the options provided, the correct answer is not listed. It seems there may be an error in the given options. Please double-check the available choices or consult your textbooks or references for further information.

I apologize for any confusion caused by the previous explanation. Let's go through it step by step to clarify.

To calculate the empirical formula, you need to determine the ratio of the moles of each element in the compound.

Given the percentages of each element:
- Carbon (C) is 54.5%
- Hydrogen (H) is 9.09%
- Oxygen (O) is 36.4%

Assuming you have 100 grams of the substance, you can convert the percentages into grams:
- C: 54.5 grams
- H: 9.09 grams
- O: 36.4 grams

Next, convert the grams into moles by dividing by the atomic mass of each element:
- Carbon's atomic mass (C) is approximately 12 g/mol, so moles of C = 54.5 g / 12 g/mol = 4.54 mol
- Hydrogen's atomic mass (H) is approximately 1 g/mol, so moles of H = 9.09 g / 1 g/mol = 9.09 mol
- Oxygen's atomic mass (O) is approximately 16 g/mol, so moles of O = 36.4 g / 16 g/mol = 2.275 mol

Next, you need to find the ratio of the moles. To do this, divide the moles of each element by the smallest number of moles. In this case, the smallest number of moles is 2.275 mol (moles of O).

Dividing the moles of each element by 2.275 mol:
- Moles of C = 4.54 mol / 2.275 mol = 2
- Moles of H = 9.09 mol / 2.275 mol = 4
- Moles of O = 2.275 mol / 2.275 mol = 1

Now you have the ratio of the moles, which represents the empirical formula of the compound: C2H4O.

The next step is to find the molecular formula, which is a whole number multiple of the empirical formula.

Given the molecular weight of the compound is 176 g/mol, you need to calculate the empirical molar mass. This is done by summing the atomic masses of each element in the empirical formula:

- Carbon (C): atomic mass = 12 g/mol, so total mass = 2 * 12 g/mol = 24 g/mol
- Hydrogen (H): atomic mass = 1 g/mol, so total mass = 4 * 1 g/mol = 4 g/mol
- Oxygen (O): atomic mass = 16 g/mol, so total mass = 1 * 16 g/mol = 16 g/mol

Summing the masses: 24 + 4 + 16 = 44 g/mol.

Dividing the molecular weight by the empirical molar mass:
- Molecular weight (176 g/mol) / empirical molar mass (44 g/mol) = 4.

Multiply the subscripts in the empirical formula (C2H4O) by this factor to obtain the molecular formula:
- C2 * 4 = C8
- H4 * 4 = H16
- O1 * 4 = O4

Therefore, the molecular formula is C8H16O4, which corresponds to option A) in the given choices.