Asample of an unknown compound was decomposed and found to be composed of 1.36 mol oxygen, 4.10 mol hydrogen, and 2.05 mol carbon. what is the empirical formula of the unknown compound? hints a sample of an unknown compound was decomposed and found to be composed of 1.36 mol oxygen, 4.10 mol hydrogen, and 2.05 mol carbon. what is the empirical formula of the unknown compound? c3h6o2 c2h4o c1.5h3o c2h3o

We are given the number of moles:

O = 1.36 mol

H = 4.10 mol

C = 2.05 mol

To get the empirical formula, first divide everything by the smallest number of moles = 1.36 mol. So that:

O = 1 mol

H = 3 mol

C = 1.5 mol

Next step is to multiply everything by a number such that all will be a whole number. In this case, multiply by 2 to get a whole number for C, so that:

O = 2 mol

H = 6 mol

C = 3 mol

Therefore the empirical formula of the compound is:

C3H6O2

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.