A compound contains 2.35% hydrogen, 14.11% carbon and 83.53% chlorine.

1.	A compound contains 2.35% hydrogen, 14.11% carbon and 83.53% chlorine. Its molar mass is 85 g / mol. What are its empirical and molecular formulas?
Answer» Explanation: step 1 Divide the given percentages of atoms with their MOLECULAR masses H---4.07/1 =4.07 C---24.27/12 =2.02 Cl--71.65/35.5=2.01 step 2 divide all VALUES with the lowest value OBTAINED. H---4.07/2.01=2 C---2.02/2.01=1 Cl---2.01/2.01=1 THEREFORE the EMPIRICAL formula is CH 2 Cl WEIGHT OF EMPIRICAL FORMULA=12+2+35.5=49.5 Given molecular weight =98.96 which is double of empirical weight .therefore molecular formula is C 2H4Cl2 .

A compound contains 2.35% hydrogen, 14.11% carbon and 83.53% chlorine. Its molar mass is 85 g / mol. What are its empirical and molecular formulas?

Answer»

Explanation:

step 1

Divide the given percentages of atoms with their MOLECULAR masses

H---4.07/1 =4.07

C---24.27/12 =2.02

Cl--71.65/35.5=2.01

step 2

divide all VALUES with the lowest value OBTAINED.

H---4.07/2.01=2

C---2.02/2.01=1

Cl---2.01/2.01=1

WEIGHT OF EMPIRICAL FORMULA=12+2+35.5=49.5

Given molecular weight =98.96 which is double of empirical weight .therefore molecular formula is C

2H4Cl2