The osmotic pressure of a solution containing 2.04 g of an unknown compound dissolved in 175.0...
The osmotic pressure of a solution containing 2.04 g of an unknown compound dissolved in 175.0 mLof solution at 25 ∘C is 2.13 atm . The combustion of 22.08 g of the unknown compound produced 36.26 g CO2 and 14.85 g H2O. What is the molecular formula of the compound (which contains only carbon, hydrogen, and oxygen)?
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The osmotic pressure of a solution containing 2.04 g of an
unknown compound dissolved in 175.0...
Combustion analysis of 0.6943 g of an unknown compound containing carbon, hydrogen, and oxygen, produced 1.471...
Combustion analysis of 0.6943 g of an unknown compound containing carbon, hydrogen, and oxygen, produced 1.471 g CO2 and 0.226 g H2O. Determine the molecular formula, given the molar mass is 166 g/ mol.
I have an unknown organic compound containing carbon, hydrogen and oxygen. Combustion analysis of 4.05 g...
I have an unknown organic compound containing carbon, hydrogen and oxygen. Combustion analysis of 4.05 g sample of the unknown produced 8.07 g CO2 and 3.76 g H2O. The molar mass of the unknown was determined to be 180 +/- 4 g/mol. What is the molecular formula of the unknown?
1.)) An unknown compound containing carbon, hydrogen and oxygen is combusted. If 25.000 g of the...
1.)) An unknown compound containing carbon, hydrogen and oxygen is combusted. If 25.000 g of the compound produced 61.024 g of CO2 and 24.981 g of H2O, what is the empirical formula of the compound? 2.)) If the molar mass of this compound is 72.1 g/mol, what is the molecular formula?
39.636 g of an unknown compound X is dissolved in 170.86 mL. What is the molarity...
39.636 g of an unknown compound X is dissolved in 170.86 mL. What is the molarity of X? Here is some information to determine the identity of X. When 1.00g of X is dissolved in water and allowed to react wtih AgNO3, all the chlorine in X precipitates and 1.95g of AgCl is collected. When 1.00g of X undergoes complete combustion, 0.900 g of CO2 and 0.735 g of H2O were collected. The empirical and molecular formula are identical. Compound...
A) The vapor pressure of an aqueous solution of potassium bromide at 31 °C is 0.04173...
A) The vapor pressure of an aqueous solution of potassium bromide at 31 °C is 0.04173 atm. The vapor pressure of pure water at the same temperature is 0.04434 atm. Estimate the freezing point of the solution. For water, Kfp = 1.86 °C/m. Answer:_____ °C B) Complete combustion of 3.769 g of a compound of carbon, hydrogen, and oxygen yielded 8.120 g CO2 and 3.325 g H2O. When 13.90 g of the compound was dissolved in 253 g of water,...
The osmotic pressure of an unknown, nonelectrolytic compound dissolved in 2.3L of solution is 8.31 atm...
The osmotic pressure of an unknown, nonelectrolytic compound dissolved in 2.3L of solution is 8.31 atm at 25 °C. How many moles of the unknown compound were dissolved? O 0.78 mol O 0.34 mol 09.3 mol O 0.15 mol
2.516 g of a compound containing carbon, hydrogen and oxygen (CXHYOZ) is subjected to combustion analysis....
2.516 g of a compound containing carbon, hydrogen and oxygen (CXHYOZ) is subjected to combustion analysis. The results show that 3.082 g of CO2 and 2.705 g of H2O were produced. (i). What is the empirical formula for the compound? (ii). If the molecular weight of the compound is 160.2 g/mol, what is the molecular formula of the compound?
Combustion of 2.78 mg of an unknown solid compound containing carbon, hydrogen and oxygen produces 6.32...
Combustion of 2.78 mg of an unknown solid compound containing carbon, hydrogen and oxygen produces 6.32 mg of CO2 and 2.58 mg H2O. What is the empirical formula of this compound?
Combustion analysis 12.01 g of an unknown sample, which contains only carbon, hydrogen and oxygen, produced...
Combustion analysis 12.01 g of an unknown sample, which
contains only carbon, hydrogen and oxygen, produced 14.08 g co2 and
4.32 h2o. Determine the empirical formula and molecular formula of
the unknown sample, while the molar mass for the unknown sample is
150.078 g/mol.
15 pts) Combustion analysis 12.01 g of an unknown sample, which contains only carbon, hydrogen, and oxygen, roduced 14.08 g CO2 and 4.32 g H20. Determine the empirical formula and molecular formula of the unknown sample,...
Complete combustion of 4.251 g of a compound of carbon, hydrogen, and oxygen yielded 6.337 g...
Complete combustion of 4.251 g of a compound of carbon, hydrogen, and oxygen yielded 6.337 g CO2 and 1.946 g H2O. When 20.30 g of the compound was dissolved in 348 g of water, the freezing point of the solution was found to be -0.919 °C. For water, Kfp = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
The osmotic pressure of an unknown, nonelectrolytic compound dissolved in 2.3L of solution is 8.31 atm at 25 °C. How many moles of the unknown compound were dissolved? O 0.78 mol O 0.34 mol 09.3 mol O 0.15 mol
Combustion analysis 12.01 g of an unknown sample, which
contains only carbon, hydrogen and oxygen, produced 14.08 g co2 and
4.32 h2o. Determine the empirical formula and molecular formula of
the unknown sample, while the molar mass for the unknown sample is
150.078 g/mol.
15 pts) Combustion analysis 12.01 g of an unknown sample, which contains only carbon, hydrogen, and oxygen, roduced 14.08 g CO2 and 4.32 g H20. Determine the empirical formula and molecular formula of the unknown sample,...
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