Acompound contains carbon, hydrogen, and nitrogen as its only elements. a 9.353 g sample of the compound contains 5.217 g of carbon and 1.095 g of hydrogen; the remainder is nitrogen. what is the empirical formula for the compound?

Empirical formular is given as ; C₂H₅N

Explanation:

Information given;

Mass of sample = 9.353g

Mass of Carbon = 5.217g

Mass of Hydrogen = 1.095g

Remainder is Nitrogen.

Mass of Nitrogen = Mass of Sample - (Mass of carbon + Hydrogen)

Mass of Nitrogen = 9.353 - (5.217 + 1.095) = 3.041g

Step 1: Determine the masses. We just calculated the value for this.

Step 2: Determine the number of moles by dividing the grams by the atomic mass.

Carbon = 5.217/12 = 0.4348

Hydrogen = 1.095/1 = 1.095

Nitrogen = 3.041/14 = 0.2172

Step 3: Divide the number of moles of each element by the smallest number of moles.

The smallest in this case is 0.2172

Carbon = 0.4348/ 0.2172 = 2.044

Hydrogen = 1.095/ 0.2172 = 5.14

Nitrogen = 0.2172/ 0.2172 = 1

Step 4: Convert numbers to whole numbers

Carbon = 2.044 = 2

Hydrogen = 5.14 = 5

Nitrogen = 1 = 1

Empirical formular is given as ; C₂H₅N

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