When 6.911 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.68 grams of CO₂ and 8.878 grams of H₂O were produced. In a separate experiment, the molecular weight of the compound was found to be 42.08 amu. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula =
When 6.911 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.68 grams of CO₂ and 8.878 grams of H₂O were produced. In a separate experiment, the molecular weight of the compound was found to be 42.08 amu. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula =
Chemistry
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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When 6.911 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.68 grams of CO₂ and 8.878 grams
of H₂O were produced.
In a separate experiment, the molecular weight of the compound was found to be 42.08 amu. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Enter the elements in the order presented in the question.
empirical formula =
96
5
molecular formula =
Sample
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[Review Topics]
[References]
Use the References to access important values if needed for this question.
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Transcribed Image Text:R
F
888
0₂
FA
When 6.911 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.68 grams of CO₂ and 8.878 grams
of H₂O were produced.
In a separate experiment, the molecular weight of the compound was found to be 42.08 amu. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Enter the elements in the order presented in the question.
empirical formula =
96
5
molecular formula =
Sample
T
[Review Topics]
[References]
Use the References to access important values if needed for this question.
G
F5
B
♫
6
stv
MacBook Air
Y
FG
H
SLA ■
&
7
N
Furnace
U
J
2
8
H₂O absorber
M
1
K
(
9
DD
FO
*
O
V
)
O
CO₂ absorber
so
F10
P
:
;
L
Previous
F11
1 +
[
=
Next
Save and Exit
F12
1
1
1
delete
1
Expert Solution
Step 1: Defining empirical and molecular formula
Answer:
Empirical formulas show the simplest whole number ratio of atoms in a compound whereas molecular formulas show the number of each type of atom in a molecule.
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