HELP ASAP I WILL GIVE BRAINLIST!! Determine the empirical formula of a compound containing 40.6 grams of carbon, 5.1 grams of hydrogen, and 54.2 grams of oxygen. In an experiment, the molar mass of the compound was determined to be 118.084 g/mol. What is the molecular formula of the compound?

For both questions, show your work or explain how you determined the formulas by giving specific values used in calculations. (10 points)

The empirical formula of the compound is: C2H3O2

The molecular formula of the compound is: C4H6O4

Explanation:

Step 1: Data given

A compound contains 40.6 grams Carbon, 5.1 grams of hydrogen and 54.2 grams of oxygen

The molar mass = 118.084 g/mol

Molar mass of carbon = 12 g/mol

Molar mass of Hydrogen = 1.01 g/mol

Molar mass of oxygen = 16 g/mol

Step 2: Calculate moles

Moles = mass / molar mass

Moles C = 40.6 grams / 12.0 g/mol = 3.38 moles

Moles H = 5.1 grams / 1.01 g/mol = 5.05 moles

Moles O = 54.2 grams / 16g/mol = 3.39 moles

Step 3: Calculate mol ratio

We divide by the smallest amount of moles

C: 3.38/3.38 = 1

H: 5.05 / 3.38 = 1.5

0: 3.39/3.38 = 1

The empirical formula is C2H3O2

The molar mass of this formula is 2*12+3*1.01+2*16 = 59.03 g/mol

Step 4: Calculate molecular formula

118.084 / 59.03 = 2

The molecular formula = 2*(C2H3O2) = C4H6O4

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