What is the empirical formula of a compound that consists of 2.424g magnesium,3.197g sulfur,and 6.380g oxygen?

Question

Quizplus · Accepted Answer

1. Calculate the moles of each element:
- Magnesium: 2.424 g / 24.31 g/mol = 0.0996 mol
- Sulfur: 3.197 g / 32.06 g/mol = 0.0996 mol
- Oxygen: 6.380 g / 16.00 g/mol = 0.3988 mol
2. Divide each mole value by the smallest value to get the mole ratio:
- Magnesium: 0.0996 mol / 0.0996 mol = 1
- Sulfur: 0.0996 mol / 0.0996 mol = 1 
- Oxygen: 0.3988 mol / 0.0996 mol = 4
3. Write the empirical formula using the mole ratio:
MgSO4/4 = MgSO1/4 = MgSOS1/4B0 = MgSOS1B14

What Is the Empirical Formula of a Compound That Consists