Question

The normal boiling point of ethanol is 351 K. It also boils at 514 K and...

The normal boiling point of ethanol is 351 K. It also boils at 514 K and 60 atm. (a) Calculate its enthalpy of vaporization in J/mol (15 points). (b) Calculate the difference in Gibbs energy between the vapor and liquid phases of ethanol at 514 K and 60 atm.

Engineering   Chemical-Engineering   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Hi here is the solution for your question. I hope I could help you in future also. If anything is not clear to you please let me know before giving your valuable feedback.

I would like to improve that in the future.

Thanks

Solution

i hope it will help you. If I missed anything or you need more explanation please let me know before giving your rating.

Thanks

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The normal boiling point of liquid ethanol is 351 K. Assuming that its molar heat of...
The normal boiling point of liquid ethanol is 351 K. Assuming that its molar heat of vaporization is constant at 45.1 kJ/mol, the boiling point of C2H5OH when the external pressure is 0.602 atm is ? K.
The normal boiling point of ethanol is 78.3oC. Assuming an average molar enthalpy of vaporization value...
The normal boiling point of ethanol is 78.3oC. Assuming an average molar enthalpy of vaporization value of 40.0 kJ/mol in the temperature interval between 20.0oC and the normal boiling point, calculate the vapor pressure of ethanol at 30.0oC.
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. Q: A) How much heat is required to convert 36.5 g of ethanol at 35 ∘C to the vapor phase at 78 ∘C? B) How much heat is required to convert 36.5 g of ethanol at -167...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅Krespectively. A. How much heat is required to convert 40.5 g of ethanol at 36 ∘C to the vapor phase at 78 ∘C? B. How much heat is required to convert 40.5 g of ethanol at -161 ∘C to...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of...
Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of vaporization is 38.56 kJ/mol. The specific heat of solid and liquid ethanol are 0.97 J/g⋅K are 2.3 J/g⋅Krespectively. A) How much heat is required to convert 26.5 g of ethanol at 34 ∘C to the vapor phase at 78 ∘C? B) How much heat is required to convert 26.5 g of ethanol at -160 ∘C to...
Ethanol (C2H5OH) boils at 78∘C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56...
Ethanol (C2H5OH) boils at 78∘C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g−K. 1. How much heat is required to convert 25.0 g of ethanol at 30 ∘C to the vapor phase at 78 ∘C? 2. Place the following substances in order of decreasing volatility: CH4, CBr4, CH2Cl2, CH3Cl, CHBr3, and CH2Br2. Rank from most volatile to least volatile. To rank items as equivalent, overlap them. 3....
A liquid has an enthalpy of vaporization of 30.8 kJ/mol. At 273 K it has a...
A liquid has an enthalpy of vaporization of 30.8 kJ/mol. At 273 K it has a vapor pressure of 102 mmHg. What is the normal boiling point of this liquid? (R = 8.31 J/(K· mol))
The normal boiling point of liquid propanol is 371 K. Assuming that its molar heat of...
The normal boiling point of liquid propanol is 371 K. Assuming that its molar heat of vaporization is constant at 43.9 kJ/mol, the boiling point of C3H7OH when the external pressure is 1.33 atm is
Trouton’s rule states that the entropy of boiling at the normal point is 85 J/mol *...
Trouton’s rule states that the entropy of boiling at the normal point is 85 J/mol * K. (a) Does the data from Example 3.2 support Trouton’s rule? (b) H2O has a heat of vaporization of 40.7 kJ/mol. Does the Delta vapS for H2O at its normal boiling point support Trouton’s rule? Can you explain any deviation? (c) Predict the boiling point of cyclohexane, C6H12, if its Delta vapH is 30.1 kJ/mol. Compare your answer to the measured normal boiling point...
The normal boiling point of ethanol is 78.3 ∘C, and the heat of vaporization is ΔHvap...
The normal boiling point of ethanol is 78.3 ∘C, and the heat of vaporization is ΔHvap = 38.6 kJ/mol. Part A What is the boiling point of ethanol in ∘C on top of Pikes Peak in Colorado, where P = 401 mmHg? Express your answer with the appropriate units.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT