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?

X_E=_____mol ethanol/mol

X_A=_____mol acetic acid/mol

Solutions

Expert Solution

queen_honey_blossom answered 2 hours ago

Next > < Previous

Related Solutions

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

how to make a mole fraction of 0.25, 0.50, 0.75 ethyl acetate and cyclohexane having a...

how to make a mole fraction of 0.25, 0.50, 0.75 ethyl acetate and cyclohexane having a total volume of 5 or 10 ml

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

Fill in the blanks NaI -- Molality = 0.25 find mass percent & mole fraction C2H5OH...

Fill in the blanks NaI -- Molality = 0.25 find mass percent & mole fraction C2H5OH -- Mass Percent = 10.0 find molality & mole fratcion C12H22O11 -- Molality = 0.15 find mass percent & mole fraction KNO3 -- Mass Percent = 5.0 find molality & mole fraction CH3COOH Molality = 0.0183 find mass percent & mole fraction

1.Given the following mole fraction and vapor pressures for miscible liquids A and B, calculate the...

1.Given the following mole fraction and vapor pressures for miscible liquids A and B, calculate the composition (in mole percentage) of the vapor from a distilling an ideal binary solution at 150°C and 760 mmHg for the solution XA=0.50 PA=1710mmHg XB=0.50 PB=130mmHg 2. Define the following. Refluxing Dalton’s Law Raoult’s Law 3. What is the mole fraction of each component if 4.0 g of benzene (C6H6) is dissolved in 6.4 g of toluene (C7H8)? 4. Consider the following solvent pairs....

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.

A single-stage liquid/vapor separation for the unknown molecule (1) and molecule (2) mixture with mole fraction...

A single-stage liquid/vapor separation for the unknown molecule (1) and molecule (2) mixture with mole fraction z1=0.75 is operated at T=100°C and P=40 kPa. Determine the partial pressure of molecule (1) in the separator. The feeding rate of the mixture is 1mole/s and the molar fraction (V) of the vapor formed is 0.5. Saturated pressure of the molecule (1) is 50.00 kPa and that of the molecule (2) is 20 kPa at the separator temperature. Assume Raoult’s law applies. (8...

Subjects