Respuesta :
Answer:
[tex]C_6H_{12}O_6[/tex]
Explanation:
Mass of water obtained = 0.0609 g
Molar mass of water = 18 g/mol
Moles of [tex]H_2O[/tex] = 0.0609 g /18 g/mol = 0.00338 moles
2 moles of hydrogen atoms are present in 1 mole of water. So,
Moles of H = 2 x 0.00338 = 0.00676 moles
Molar mass of H atom = 1.008 g/mol
Mass of H in molecule = 0.00676 x 1.008 = 0.00681 g
Mass of carbon dioxide obtained = 0.1486 g
Molar mass of carbon dioxide = 44.01 g/mol
Moles of [tex]CO_2[/tex] = 0.1486 g /44.01 g/mol = 0.00337 moles
1 mole of carbon atoms are present in 1 mole of carbon dioxide. So,
Moles of C = 0.00337 moles
Molar mass of C atom = 12.0107 g/mol
Mass of C in molecule = 0.00337 x 12.0107 = 0.04047 g
Given that the compound only contains hydrogen, oxygen and carbon. So,
Mass of O in the sample = Total mass - Mass of C - Mass of H
Mass of the sample = 0.1014 g
Mass of O in sample = 0.1014 - 0.04047 - 0.00681 = 0.05412 g
Molar mass of O = 15.999 g/mol
Moles of O = 0.05412 / 15.999 = 0.00338 moles
Taking the simplest ratio for H, O and C as:
0.00676 : 0.00338 : 0.00337
= 2 : 1 : 1
The empirical formula is = [tex]CH_2O[/tex]
Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.
Thus,
Molecular mass = n × Empirical mass
Where, n is any positive number from 1, 2, 3...
Mass from the Empirical formula = 1×12 + 2×1 + 16= 30 g/mol
Molar mass = 180 g/mol
So,
Molecular mass = n × Empirical mass
180 = n × 30
⇒ n = 6
The formula of compound = [tex]C_6H_{12}O_6[/tex]
As the 0.1014 gram of a sample of the purified CHO. The compound was burned in a combustion and apparatus and was made form the 0.1486 g CO2 and 0.0609 g of H2O.
- Mass of water obtained = 0.0609 g Molar mass of water = 18 g/mol Moles of = 0.0609 g /18 g/mol = 0.00338 moles . 2 moles of hydrogen atoms are present in 1 mole of water. So, Moles of H = 2 x 0.00338 = 0.00676 moles
- Molar mass of carbon dioxide = 44.01 g/mol . Moles of = 0.1486 g /44.01 g/mol = 0.00337 moles, Mass of water obtained = 0.0609 gMolar mass of water = 18 g/mol
Learn more about the purified CHO compound was burned.
brainly.com/question/14547037.
