Question

an organic compound contains 4.075% of hydrogen,24.27 ℅of carbon,71.65℅ of chlorine.calculate the empirical formula and molecular formula. the molecular mass of the compound is 98.96g​

Answer 1

Answer:

The empirical formula is CH2Cl . The molecular formula is  C 2 H 4 Cl 2 .

Explanation:

The empirical formula is the simplest whole-number ratio of atoms in a compound.  

The ratio of atoms is the same as the ratio of moles.

So, our job is to calculate the molar ratio of  C  to  H  to  Cl .  Your compound contains 24.27 %  C , and 4.07 %  H .  Assume that you have 100 g of sample.  

Then it contains 24.27 g of  C and 4.07 g of  H .  

Mass of O = (100 - 24.27 - 4.07) g = 71.66 g

Moles of C = 24.27 g C × 1 mol C 12.01 g C = 2.021 mol C

Moles of H = 4.07 g H × 1 mol H 1.008 g H = 4.038 mol H

Moles of Cl = 71.66 g Cl × 1 mol Cl 35.45 g Cl = 2.021mol Cl

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