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)

Empirical Formula C₂H₅O₂

Molecular Formula C₄H₁₀O₄

Explanation:

To calculate empirical formula use the periodic table to convert the given masses to moles. Then, divide by the smallest number of moles calculated and round (1.9 = 2) multiply if needed to get the lowest whole number ratio (in cases where the number is 2.5 or something similar). This will be the empirical formula.

To calculate molecular formula use the periodic table to find the molar mass of the empirical number, then divide the given amount by the amount you have calculated. This whole number will be what you should multiply the subscripts of the empirical formula by to get the molecular formula.

See attached image for work.

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explanation:

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