A4.647 g of white solid contain only c, h and o is completely burned with excess of oxygen to produce 8.635 g of co2 and 1.767 g of h2o. what is empirical formula of the compound?

EMPIRICAL FORMULA:

C₂H₃O₂

Explanation:

Mass of compound = 4.647 g

Mass of CO₂ = 8.635 g

Mass of H₂O = 1.767 g

Empirical formula = ?

Solution:

Percentage of C = 8.635/ 4.647 × 12/44 ×100

Percentage of C = 1.86× 12/44 ×100 = 50.7

Percentage of H = 1.767/4.647 × 2/ 18 × 100

Percentage of H = 0.38 × 2/ 18 × 100

Percentage of H = 4.18

Percentage of O = 100 - (50.7+4.18)

Percentage of O = 100 - 54.88

Percentage of O = 45.12

Number of grams atom:

Number of grams atom of C = 50.7/ 12 = 4.23

Number of grams atom of H = 4.18 /1 = 4.18

Number of grams atom of O = 45.12/ 16 = 2.82

Atomic ratio:

            C            :          H                :            O

     4.23/2.82     :         4.18/2.82    :            2.82/2.82

         1                :              1.5          :                1

C :  H  :  O    (1 : 1.5 : 1)

C :  H  :  O    2(1 : 1.5 : 1)

C :  H  :  O    (2 : 3 : 2)

EMPIRICAL FORMULA:

C₂H₃O₂

it is b that is the answer.