Question

A compound with the empirical formula SO has a molecular weight of 96.13 amu. The molecular formula is S_O_

Answer 1

The molecular formula of the compound with the empirical formula SO and a molecular weight of 96.13 amu is S2O2 or SO2.

Step-by-step explanation:

The molecular formula of a compound can be determined from its empirical formula and molecular weight. In this case, the compound has an empirical formula of SO and a molecular weight of 96.13 amu. To find the molecular formula, we need to compare the ratio of the empirical formula mass to the molecular mass. The empirical formula mass of SO can be calculated by adding the atomic masses of sulfur (32.07 amu) and oxygen (16.00 amu), which gives a total of 48.07 amu.

To find the molecular formula, we divide the molecular weight by the empirical formula mass. In this case, 96.13 amu / 48.07 amu = 2. So, the empirical formula needs to be multiplied by 2 to get the molecular formula. Therefore, the molecular formula is S2O2 or SO2.

Answer 2

Molecular mass / empirical mass = number with with the empirical formula needs to be multiplied to get molecular formula

Empirical mass = Atomic mass of S + atomic mass of O = 32.07 + 16 = 48.07

molar mass = 96.13 g

So ratio = 96.13 / 48.07 = 2

Hence the molecular formula = S2O2