If a compound has a molar mass of 180 g/mol and its empirical formula is CH20, what is its molecular formula?

CH20

C2H402

O C6H1206

C12H22011

C6H12O6

Explanation:

The empirical formula is CH2O

The molecular formula is n times the empirical formula CH2O. With n = 1,2,3, ...

n = the ratio between molar mass / mass of the empirical formula

The empirical formula CH2O has:

C ⇒ 12g/mole

H2 ⇒ 2*1g/mole = 2g/mole

O = 16g/mole

12+2+16 : 30g/mole

Molar mass of the compound = 180g/mole

⇒n = ratio between molar mass / mass of the empirical formula

n = 180/30 = 6

This means we have to multiply each element by 6

6C

12H

6O

The molecular formula is C6H12O6

If we control this: 6*12 + 12*1 + 6*16 = 72+12+96 = 180g/mole

This compound is probably glucose (or fructose)