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.

Empirical Formula:

The empirical formula of a compound is the simplest whole-number ratio of the numbers of the different atoms that compose the molecule of the compound. The empirical formula looks like a molecular formula.

C

2

H

2

and

C

H

are the molecular formula and the empirical formula of acetylene.

The Given Data

The mass of carbon in the compound:

m

C

=

40.6

g

The mass of hydrogen in the compound: {eq}m_H = 5.1 \ \rm...

C4H6O, C2H3O2

Explanation:

C:H:O                                                            C2H3O2

40.6:5.1:54.2                                                (12x2) + (1x3) + (16x2) = 59

40.6/12 : 5.1/1 : 54.1/16                              118.1/59 =2     

3.38 : 5.1 : 3.38                                            C4H6O4

X (1:1.5:1) =

C2H3O2

i'm assuming that it's c.) red bank..