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 second step is to calculate the number of moles of each element present in the sample. To do this, you must divide the mass of each element by its molar mass. The masses of the elements present are: mass H = g mass S = g mass O = g

Question

Chemistry

Phoenix

1 July, 01:06

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 second step is to calculate the number of moles of each element present in the sample. To do this, you must divide the mass of each element by its molar mass. The masses of the elements present are: mass H = g mass S = g mass O = g

+2

Answers (2)

Know the Answer?

Quintin Hancock · Answer 1

the masses of the elements present are:

mass H = 2.00 g

mass S = 32.7 g

mass O = 65.3 g

Konner Nelson · Answer 2

Lets take 100 g of this compound,

so it is going to be 2.00 g H, 32.7 g S and 65.3 g O.

2.00 g H * 1 mol H/1.01 g H ≈ 1.98 mol H

32.7 g S * 1 mol S / 32.1 g S ≈ 1.02 mol S

65.3 g O * 1 mol O/16.0 g O ≈ 4.08 mol O

1.98 mol H : 1.02 mol S : 4.08 mol O = 2 mol H : 1 mol S : 4 mol O

Empirical formula

H2SO4