Question
In: Chemistry
1)When 5.352 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.38 grams...
1)When 5.352 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 18.38 grams of CO2 and
3.010grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 128.2 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
2)When 4.948 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 16.72 grams of CO2 and
3.424grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 26.04 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
When 5.895 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.50 grams...
When 5.895 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 18.50 grams of CO2and
7.574 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 42.08 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Empirical formula?
Molecular formula?
When 6.597 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.74 grams...
When 6.597 grams of a hydrocarbon, CxHy, were burned in a
combustion analysis apparatus, 21.74 grams of CO2 and 5.935 grams
of H2O were produced. In a separate experiment, the molar mass of
the compound was found to be 40.06 g/mol. Determine the empirical
formula and the molecular formula of the hydrocarbon.
When 6.104 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.15 grams...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a
combustion analysis apparatus, 19.15 grams of CO2 and 7.842 grams
of H2O were produced. In a separate experiment, the molar mass of
the compound was found to be 28.05 g/mol. Determine the empirical
formula and the molecular formula of the hydrocarbon.
A 7.797 gram sample of an organic compound
containing C, H and O is analyzed by combustion analysis and
7.623 grams of CO2 and
1.561 grams of H2O...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 19.15 grams...
When 6.104 grams of a hydrocarbon, CxHy, were burned in a
combustion analysis apparatus, 19.15 grams of CO2 and 7.842 grams
of H2O were produced. In a separate experiment, the molar mass of
the compound was found to be 28.05 g/mol. Determine the empirical
formula and the molecular formula of the hydrocarbon.
A 7.797 gram sample of an organic compound containing C, H and O
is analyzed by combustion analysis and 7.623 grams of CO2 and 1.561
grams of H2O...
When 1.661 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 5.211grams of...
When 1.661 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 5.211grams of CO2 and
2.134 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 42.08 g/mol. Determine the empirical formula
and the molecular formula of the hydrocarbon.
Enter the elements in the order presented in the question.
5a. When 4.355 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 14.72...
5a. When 4.355 grams of a hydrocarbon,
CxHy, were burned in a combustion analysis
apparatus, 14.72 grams of CO2 and
3.014 grams of H2O were produced.
In a separate experiment, the molar mass of the compound was found
to be 26.04 g/mol. 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 =
5b.
A 12.57 gram sample of an organic compound
containing C,...
when 4.027 grams hydrocarbon, CxHy, we're burned in a combustion analysis apparatus, 12.64 grams of CO2...
when 4.027 grams hydrocarbon, CxHy, we're burned in a
combustion analysis apparatus, 12.64 grams of CO2 and 5.174 grams
H2O we're produced.
I need empirical and molecular formulas
As with any combustion reaction, the products of combusting a hydrocarbon fuel (CxHy) with oxygen (O2)...
As with any combustion reaction, the products of combusting a
hydrocarbon fuel (CxHy) with oxygen (O2) are carbon dioxide (CO2)
and water (H2O).
A mass of 16.89 g for an unknown fuel was combusted in
a reaction vessel containing an unknown amount of oxygen. At the
end of the reaction, there still remained 16.85 g of the fuel as
well as 0.0654 g of water and 0.1198 g of carbon dioxide. The
oxygen was completely consumed during the reaction.
How...
A high grade fuel oil which consists of only hydrocarbon, CxHy is burnt in a combustion...
A high grade fuel oil which consists of only hydrocarbon, CxHy
is burnt in a combustion chamber at 25 °C. The standard heat of
combustion is -43,515 J/g with CO2 (g) and H2O (l) as products. The
temperature of the fuel and air entering the combustion chamber is
25 °C. The air is assumed dry. The flue gases leave at 300 °C and
their average composition is 11.2 % CO2, 0.4 % CO, 6.2 % O2 and
82.2 % N2...
Complete combustion of a 0.0150 mol sample of a hydrocarbon, CxHy, gives 3.024 L of CO2...
Complete combustion of a 0.0150 mol sample of a hydrocarbon,
CxHy, gives 3.024 L of CO2 at STP and 1.891 g of H2O.
(a) What is the molecular formula of the hydrocarbon?
(b) What is the empirical formula of the hydrocarbon?
A 0.500-L bulb containing Ne at 685 torr is connected by a valve
to a 2.50-L bulb containing CO2 at 375 torr. The valve between the
two bulbs is opened and the two gases mix. The initial gas
pressures...
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