Question

Determine the molecular formula for the following compounds from the experimental data:-37.5% carbon, 6.3% hydrogen, 55.8% chlorine, and molecular mass of 127.0 amu

Answer 1

`C_4H_8Cl_4`

Explanations:

Given the following compounds from the experimental data:

Carbon = 37.5%

Hydrogen = 6.3%

Chlorine = 55.8%

Convert to mass

Carbon = 37.5g

Hydrogen = 6.3g

Chlorine = 55.8g

Covert the mass to moles

Moles of C = 37.5/12 = 3.125moles

Moles of H = 6.3/1 = 6.3moles

Moles of Cl = 55.8/17 = 3.282moles

Divide by the lowest number of moles

For Carbon: 3.125/3.125 = 1

For Hydrogen: 6.3/3.125 = 2.016

For Chlorine: 3.282/3.125 = 1.05 moles

Determine the empirical formula

CH2Cl

Determine the molecular formula

(CH2Cl)n = 127

(12 + 2 + 17)n = 127

31n = 127

n = 127/31

n = 4.09 = 4

The molecular formula will be (CH2Cl)4 = C4H8Cl4