Just making sure I\'m doing this right: Given .2217g of an unknown solute broken

Question

Just making sure I'm doing this right:
Given .2217g of an unknown solute broken down as: 85.7% C, 5.53% H, 8.78% O
I have to figure out the empirical formula, molecular mass, and molecular formula.

I mostly didn't round down until the end
For the empirical formula:
.2217g of solute
85.7% C would be .18699969g C x 1 mol C/12.012g C = .0158 mol C
5.53% H would be .01226001g H x 1 mol H/1.0079g H = .0122 mol H
8.78% O would be .01946526g O x 1 mol O/15.9994g O = .0012 mol O

.0158/.0012 = 13
.0122/.0012 = 10
.0012/.0012 = 1

So the empirical formula is C13H10O?

Then for the molecular mass:
C 13 x 12.012 = 156.156
H 10 x 1.0079 = 10.079
O 1 x 15.9994 = 15.9994

= 182.2344 g/mol


Molecular Formula:

C 12.012 + H 1.0079 + O 15.9994 = 29.0193
182.2344/29.0193 = 6
C13H10O x 6 = C78 H60 O6

Am I doing this correctly?

Explanation / Answer

correct

Related Questions

Navigate

• Browse (All)
• Browse J
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.