Question

Question (a)Calculate the empirical formula of a compound that has the following composition by mass. 29.0% Na, 40.5% S, and the remainder being oxygen.

Question b:
If the molecular mass of the compound in question(a) is found to be 158 g/mol, what is the molecular formula of the compound?

For question A I got NaSO2 is that right?

Answer 1

Empirical formula is Na₂S₂O₃.

Molecular formula = Na₂S₂O₃

Step-by-step explanation:

Given data:

Percentage of sodium = 29.0%

Percentage of sulfur = 40.5%

Molecular formula = ?

Empirical formula = ?

Solution:

Number of gram atoms of Na = 29.0/23 =1.261

Number of gram atoms of S = 40.5 / 32 = 1.266

Number of gram atoms of O = 30.5 / 16 = 1.906

Atomic ratio:

Na : S : O

1.261/1.261 : 1.266/1.261 : 1.906/1.261

1 : 1 : 1.5

Na : S : O = 2 ( 1: 1 : 1.5)

Na : S : O = 2 : 2 : 3

Empirical formula is Na₂S₂O₃.

Molecular formula:

Molecular formula = n (empirical formula)

n = molar mass of compound / empirical formula mass

n = 158 / 158

n = 1

Molecular formula = n (empirical formula)

Molecular formula = 1 (Na₂S₂O₃)

Molecular formula = Na₂S₂O₃