What is the molecular formula of the compound with a molecular weight of 112 g/mol and percent composition: 85.6% c and 14.4 % h

The molecular formula is C8H16

Explanation:

Step 1: Data given

The molecular weight = 112 g/mol

The compoun contains 85.6 % C and 14.4 % H

Step 2: Calculate mass of C and H

Let's consider 100 gram of this compound

⇒ 85.6 % of C = 85.6 grams of C

⇒ 14.4 % of H = 14.4 grams of H

Step 3: Calculate moles of C

Moles C = Mass C / molar mass C

Moles C = 85.6 grams / 12.0 g/mol

Moles C = 7.13 mol

Step 4: Calculate moles of H

Moles H = 14.4 grams / 1.01 g/mol

Moles H = 14.3 moles

Step 5: Calculate the mol ratio

We divide by the smallest amount of moles

C: 7.13/7.13 = 1

H: 14.3 / 7.13 = 2

The empirical formula is CH2

The molar mass of the empirical formula is 14.02 g/mol

Step 6: Calculate the molecular formula

We have to multiply the empirical formua by n

n = 112 g/mol / 14.02 g/mol

n = 8

The molecular formula is C8H16

because u need two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their nuclei to form isotopes.

so since they all have the same shape? i mean maybe because m& m and reeses are both chocolates