Advertisements
Advertisements
Question
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Calculate the mass of carbon contained in this quantity of carbon dioxide and thus the mass of carbon in sample X.
Advertisements
Solution
Molecular weight of carbon dioxide (CO2) = 12 x 2 x 16 = 44
According to mole-concept, mass of carbon in 44 g
∴ 1 mole of CO2 = 12 g
∴ Mass of carbon in 0.01 mole of CO2 = 12 x 0.01 g
= 0.12 g
APPEARS IN
RELATED QUESTIONS
The equation for the burning of octane is:
\[\ce{2C8H18 + 25O2 -> 16CO2 + 18H2O}\]
What is the empirical formula of octane?
An organic compound contains H = 4.07%, Cl = 71.65% chlorine and remaining carbon. Its molar mass = 98.96. Find its empirical formula.
A hydrocarbon contains 4.8g of carbon per gram of hydrogen. Calculate:
find the empirical formula.
Determine the formula of the organic compound if its molecule contains 12 atoms of carbon. The percentage compositions of hydrogen and oxygen are 6.48 and 51.42 respectively.
10.47 g of a compound contained 6.25 g of metal A and rest non-metal B. Calculate the empirical formula of the compound [At. wt of A = 207, B = 35.5]
A hydride of nitrogen contains 87.5% percent by mass of nitrogen. Determine the empirical formula of this compound.
An experiment showed that in a lead chloride solution, 6.21 g of lead is combined with 4.26 g of chlorine. What is the empirical formula of this chlorine? (Pb = 207; Cl = 35.5)
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Calculate the number of moles of carbon dioxide gas.
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Calculate the mass of hydrogen in sample X.
The following experiment was performed in order to determine the formula of a hydrocarbon. The hydrocarbon X is purified by fractional distillation.
0.145 g of X was heated with dry copper (II) oxide and 224 cm3 of carbon dioxide was collected at S.T.P.
Calculate the empirical formula of X by the following step:
Deduce the ratio of atoms of each element in X (empirical formula).
