Question

1. An organic compound containing carbon, hydrogen and oxygen was analyzed that the mass percentage of...

1. An organic compound containing carbon, hydrogen and oxygen was analyzed that the mass percentage of each was found to be 49.99 % for carbon, 5.48 % for hydrogen, and 44.53 % for oxygen. Find out the empirical formula of this organic compound. 2. For the question 1, if the molecular weight of the compound was found to be 112.13 g/mol, what is the molecular formula of this compound?

First, assume 100 g of sample

so

49.99 g of C

5.48 g of H

44.53 g of O

change to mol

MW of C = 12, MW of H = 1, MW of O = 16

mol of C = mass/MW = 49.99/12 = 4.16583

mol of H = mass/MW = 5.48/1 = 5.48

mol of O = mass/MW = 44.53/16 = 2.783125

ratio:

H:C = 5.48/4.16583 = 1.3 or 4:3

H:O 5.48/2.783125= 1.96 or 2

the nearest empiricalformula:

C3H4O2

if MW of molecular compound = 12*3 + 4*1 + 16*2 = 72 g/mol

ratio = 112.13/72 = 1.5x

so

C3H4O2 * 1.5 = C4.5H6O3

nearest vlaue will be C5H6O3