Question
In: Chemistry
1a) A 2.95 g sample of an unknown chlorofluorocarbon (an organic compound containing chlorine and fluorine)...
1a) A 2.95 g sample of an unknown chlorofluorocarbon (an organic compound containing chlorine and fluorine) is decomposed and produces 581 mL of chlorine gas at a pressure of 752 mmHg and a temperature of 298 K. What is the percent by mass of chlorine in the chlorofluorocarbon?
1b) Calculate the density of Freon-11 (CFCl3) at 118 °C and 7.20 atm
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
A 2.95 g sample of an unknown chlorofluorocarbon is decomposed and produces 579 mL of chlorine...
A 2.95 g sample of an unknown chlorofluorocarbon is decomposed
and produces 579 mL of chlorine gas at a pressure of 756 Torr and a
temperature of 298 K. Part A What is the percent chlorine (by mass)
in the unknown chlorofluorocarbon?
you are analyzing an unknown organic compound in the lab. the sample of unknown organic compound...
you are analyzing an unknown organic compound in the lab. the
sample of unknown organic compound has a mass of 18.8 grams. you
decide to determine the emprirical formula of the unknown compound
using combustion analysis. after combustion, you find that 27.6
grams of carbon dioxide and 11.3 grams of waer have been produced.
what is the empirical formula for the unknown organic compound?
Combustion of a 0.525g sample of an unknown organic compound containing only C, H, and O...
Combustion of a 0.525g sample of an unknown organic compound
containing only C, H, and O yielded 1.113g CO2 and 0.1708g of H20.
What is the emperical formula of the compound? If the molar mass of
the compound is 166.13g/mol, what is the molecular formula?
Please show work!!!!
1a. A 9.236 gram sample of an organic compound containing C, H, and O is analyzed...
1a.
A 9.236 gram sample of an organic compound containing C, H, and O
is analyzed by combustion analysis and 13.10 grams of CO2 and 8.044
grams of H2O are produced. In a separate experiment, the molar mass
is found to be 62.07g/mol. Determine the emperical and molecular
formula of the organic compound.
1b. A 2.743 gram sample of an organic compound containing C,
H, and O is analyzed by combustion analysis and 6.236 grams of CO2
and 2.553 grams...
A sample of 0.7960 g of an unknown compound containing barium ions (Ba2+) is dissolved in...
A
sample of 0.7960 g of an unknown compound containing barium ions
(Ba2+) is dissolved in water and treated with an excess of Na2SO4.
If the mass of the BaSO4 precipitate formed is 0.7651 g, what is
the percent by mass of Ba in the original unknown compound?
————————
How many grams of NaCl are required to precipitate most of the
Ag+ ions from 2.50 × 102 mL of 0.0467 M AgNO3 solution
———
How many grams of KHP are...
When a 0.860 g sample of an organic compound containing C, H, and O was burned...
When a 0.860 g sample of an organic compound containing C, H,
and O was burned completely in oxygen, 1.64 g of CO2 and
1.01 g of H2O were produced. What is the empirical
formula of the compound?
Combustion analysis of a 13.42-g sample of the unknown organic compound (which contains only carbon, hydrogen,...
Combustion analysis of a 13.42-g sample of the unknown organic
compound (which contains only carbon, hydrogen, and oxygen)
produced 39.61 g CO2 and 9.01 g H2O. The molar mass of the unknown
compound is 268.34 g/mol . Find the molecular formula of the
unknown compound.
Combustion analysis of a 13.42-g sample of the unknown organic compound (which contains only carbon, hydrogen,...
Combustion analysis of a 13.42-g sample of the unknown
organic compound (which contains only carbon, hydrogen, and oxygen)
produced 39.61 g CO2 and 9.01 g H2O. The molar mass of equilin is
268.34 g/mol. Find the molecular formula of the unknown compound.
Express your answer as a chemical formula.
Combustion analysis of a 13.42-g sample of the unknown organic compound (which contains only carbon, hydrogen,...
Combustion analysis of a 13.42-g sample of the unknown organic
compound (which contains only carbon, hydrogen, and oxygen)
produced 36.86g CO2 and 10.06g H2O. The molar mass of estriol is
288.38g/mol .
Find the molecular formula of the unknown compound
1. Chlorine and fluorine gases can react to form chlorine trifluoride: Cl2(g) + 3F2(g) -->...
1. Chlorine and fluorine gases can react to form chlorine
trifluoride: Cl2(g) + 3F2(g)
--> 2ClF3(g)
What is the theoretical yield in grams of chlorine trifluoride
(ClF3)if a 2.0 L container at 350 K initially contains
Cl2 gas at a partial pressure of 1.0 atm and fluorine
gas at a partial pressure of 2.0 atm?
Hint: This is a limiting reactant problem.
A.
8.6 g ClF3
B.
21.5 g ClF3
C.
13 g ClF3
D.
19.3 g ClF3
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