A 4.647 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?

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Respuesta :

Neetoo Neetoo · Answer 1 · 2019-11-16T14:23:50+01:00

Answer:

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