Question

A compound is 2.00% H by mass, 32.7% S by mass, and 65.3% O by mass. What is its empirical formula? The first step is to calculate the mass of each element in a 100-g sample of the compound. We use 100 g because it makes the calculations more straightforward. What is the mass of each element in a 100.0-g sample of the compound? mass H = g mass S = g mass O = g

Answer 1

For a 100-g compound, we would have 2 g H, 32.7 g S, and 65.3 g O. We then divide each of these masses by their molar masses:
2 g H / 1.01 g/mol = 1.98 mol H
32.7 g S / 32.07 g/mol = 1.0196 mol S
65.3 g O / 16.00 g/mol = 4.08125 mol O
We then divide each amount of moles by the smallest of them, which is the 1.0196 from S:
1.98 mol H / 1.0196 mol S = 1.94 H ~ 2 H
1.0196 mol S / 1.0196 mol S = 1 S
4.08125 mol O / 1.0196 mol S = 4 O
So the empirical formula of the compound is H2SO4.

Answer 2

Answer:

2.00

32.7

65.3

in order

Explanation: