First take all percents and make them grams. Since you're not given a overall molar mass you can assume it is 100 and therefore the percents are their masses.
So you have 14.31g Carbon, 1.2g Hydrogen, and 84.49g of Chlorine. Next you divide each by their molar masses to get moles of each.

Carbon= 14.31g Hydrogen= 1.2g Chlorine= 85.49g
12.01g 1.01g 35.45g
= 1.19moles = 1.188moles = 2.411moles

Next you divide each of those numbers by the smallest, in this case, Hydrogen.
Thus,
Carbon= 1.19moles Hydrogen= 1.188moles Chlorine= 2.411moles
1.188moles 1.188moles 1.188moles
=1.002 =1 =2.02
These are all close enough to round, so your final empirical formula is: CHCl2
Hope that helps!!

6 0

3 years ago

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, w

Leviafan [203]

PV = constant

V doubles, P will become half

New pressure = 100/2 = 50 torr

6 0

3 years ago