Question

In: Other

A vapor composed of 0.65 mole fraction ethanol and 0.35 mole fraction acetic acid at 120.0...

A vapor composed of 0.65 mole fraction ethanol and 0.35 mole fraction acetic acid at 120.0 mmHg (absolute), is in equilibrium with a liquid phase also composed of ethanol and acetic acid. Assume that the liquid is an ideal solution and apply Raoult's law to find the following.

What is the temperature of the liquid____oC?

What are the mole fractions of the liquid pahse?

XE=___mol ethanol/mol

XA=___ mol acetic acid/mol

Solutions

Expert Solution

Amanda K answered 2 years ago
Next > < Previous

Related Solutions

Chemical Engineering Problem: A vapor composed of 0.25 mole fraction ethanol and 0.75 mole fraction acetic...
Chemical Engineering Problem: A vapor composed of 0.25 mole fraction ethanol and 0.75 mole fraction acetic acid at 120.0 mmHg (absolute), is in equilibrium with a liquid phase also composed of ethanol and acetic acid. Assume that the liquid is an ideal solution and apply Raoult\'s law to find the following. What is the temperature of the liquid? What is the Temperature of the fluid? _____C What are the mole fractions of the liquid phase? XE=_____mol ethanol/mol XA=_____mol acetic acid/mol
How much energy per mole is required to transfer acetic acid, a byproduct of ethanol metabolism...
How much energy per mole is required to transfer acetic acid, a byproduct of ethanol metabolism from blood to urine. The relevant concentrations are 39.00 and 742.00 ppm respectively and you are running a fever at 39oC. State your answer in kJ/mol. (Donnan Potential Question) EDIT: ITS ASKING FOR HOW MUCH ENERGY IN KJ/MOL IS NEEDED TO TRANSPORT ACETIC ACID FROM BLOOD TO URINE.
How much energy per mole is required to transfer acetic acid, a byproduct of ethanol metabolism...
How much energy per mole is required to transfer acetic acid, a byproduct of ethanol metabolism from blood to urine. The relevant concentrations are 33.00 and 674.00 ppm respectively and you are running a fever at 39oC. State your answer in kJ/mol.
What is the vapor pressure of a 34.6 g sample of ethanol (C2H5OH) in 120.0 mL...
What is the vapor pressure of a 34.6 g sample of ethanol (C2H5OH) in 120.0 mL of water if the vapor pressure of water is 24.4 mmHg and the density is 0.9945 g/mL? Answer choices: A. 0.751 atm B. 0.0288 atm C. 21.9 atm D. 6.99 atm
What is the mole fraction of water in a solution containing water and ethanol that is...
What is the mole fraction of water in a solution containing water and ethanol that is 470% water by mass?
Determine the mole fraction of ethanol when 8.8 moles of ethanol are dissolved in 9.56 moles...
Determine the mole fraction of ethanol when 8.8 moles of ethanol are dissolved in 9.56 moles of water. Answer to 3 decimal places. Determine the mole fraction of ethanol, C2H5OH (Molar mass = 46.08 g/mol) when 12 grams of ethanol is dissolved in 43.3 grams of water, H2O (Molar mass = 18.02 g/mol). Answer to 3 decimal places. Determine the molarity of a solution that contains 1.5 moles of ethanol dissolved in 9.7 liters of solution. Answer to 2 decimal...
What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of...
What is the mole fraction of ethanol in a solution made by dissolving 29.2 g of ethanol, C2H5OH, in 53.6 g of water? 0.176 0.213 0.545 0.352
What are the mole fraction (X) and molality (m) of ethanol (C2H5OH) in an aqueous solution...
What are the mole fraction (X) and molality (m) of ethanol (C2H5OH) in an aqueous solution that is 45.0% ethanol by volume? The density of water is 1.00 g/mL and that of ethanol is 0.789 g/mL. mole fraction = ?????; molality = ??? m
Draw the structures of ethanol and acetic (ethanoic) acid in the ground and conjugate acid states...
Draw the structures of ethanol and acetic (ethanoic) acid in the ground and conjugate acid states and then account why acetic acid is a stronger acid than ethanol.
Part A Calculate the pH of 0.376 L of a 0.18 M acetic acid - 0.35...
Part A Calculate the pH of 0.376 L of a 0.18 M acetic acid - 0.35 M sodium acetate buffer before and after the addition of 0.0065 mol of KOH. Assume that the volume remains constant. (Ka of acitic acid is 1.8⋅10−5) Express your answer using three significant figures. Part B Calculate the pH of 0.376 L of a 0.18 M acetic acid - 0.35 M sodium acetate buffer before and after the addition of 0.0065 mol of HBr. Assume...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT