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zalisa [80]
3 years ago
12

A sample in the laboratory is found to contain 3.36 grams of hydrogen, 20.00 grams of carbon, and 26.64 grams of oxygen. The mol

ecular mass is 180.156 g/mol. Determine both the empirical formula and the molecular formula.
Chemistry
1 answer:
KonstantinChe [14]3 years ago
5 0

Answer:

Empirical formula is CH₂O.

Molecular formula = C₆H₁₂O₆

Explanation:

Given data:

Mass of hydrogen = 3.36 g

Mass of carbon = 20.00 g

Mass of oxygen = 26.64 g

Molar mass of compound = 180.156 g/mol

Empirical formula = ?

Molecular formula = ?

Solution:

Empirical formula:

It is the simplest formula gives the ratio of atoms of different elements in small whole number

Number of gram atoms of H = 3.36 / 1.01 = 3.3

Number of gram atoms of O = 26.64 / 16 = 1.7

Number of gram atoms of C = 20 / 12 = 1.7

Atomic ratio:

            C                      :        H            :         O

           1.7/1.7                :     3.3/1.7       :       1.7/1.7

              1                     :           2          :        1

C : H : O = 1 : 2 : 1

Empirical formula is CH₂O.

Molecular formula:

Molecular formula = n (empirical formula)

n = molar mass of compound / empirical formula mass

Empirical formula mass = CH₂O = 12×1 + 2× + 16

Empirical formula mass = 30

n = 180.156 / 30

n = 6

Molecular formula = n (empirical formula)

Molecular formula = 6 (CH₂O)

Molecular formula = C₆H₁₂O₆

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Use the question marck Moles of CO2
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Always start with the giving

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___________  / _____________ = Cancel the queal ( O2)
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You should look at the giving number ( how many num u gor ever there) 
Ur answer should have the same # as ur givin so 
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