A compound is 2.00% H by mass, 32.7% S by mass, and 853% O by mass. What is its empirical

formula?

The final step is to use the mole ratios of the elements to write the empirical formula

The mole ratios of the elements are:

mole ratio of H:S:0 = 2:14

The mole ratios show the ratios of the elements in the compound. Use these ratios to identify the

subscripts on each element in the empirical formula Remember that the subscript 1 is not shown

What is the correct empirical formula for this compound?

HSO

H₂SO4

H2SO4

Question

Alena Zhang

Chemistry

28 July, 08:13

A compound is 2.00% H by mass, 32.7% S by mass, and 853% O by mass. What is its empirical

formula?

The final step is to use the mole ratios of the elements to write the empirical formula

The mole ratios of the elements are:

mole ratio of H:S:0 = 2:14

The mole ratios show the ratios of the elements in the compound. Use these ratios to identify the

subscripts on each element in the empirical formula Remember that the subscript 1 is not shown

What is the correct empirical formula for this compound?

HSO

H₂SO4

H2SO4

+2

Answers (1)

Know the Answer?

Chewy · Answer 1

H2SO4

Explanation:

In 100 g of the compound we hgave

2.00 g H, 32.7 g S and 65.3 g O.

2g * 1 mol/g = 2.0 mol H

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

65.3 g 0 * 1 mol/16 g = 4.08 mol O

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

H2SO4