Question

Use the thermodynamic data provided below to determine ΔG (in kJ/mol) for the condensation of C2H5OH...

Use the thermodynamic data provided below to determine ΔG (in kJ/mol) for the condensation of C2H5OH at 64.02 °C if the initial partial pressure of C2H5OH is 1.99 atm. Report your answer to one decimal place in standard notation (i.e. 123.4 kJ/mol).

Substance ΔH°f (kJ/mol) S° (J mol-1K-1)
C2H5OH (l) -277.7 160.7
C2H5OH (g) -235.1 282.7

Homework Answers

Answer #1

For C2H5OH (l)

G = H - TS

G = -277.7 kJ/mol - 337.02 (0.1607kJ mol-1K-1)

G = -331.85 kJ mol-1

For C2H5OH (g)

G = H - TS

G = -235.1 kJ mol-1- 337.02 (0.2827kJ mol-1K-1)

G = -330.375 kJ mol-1

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Use the thermodynamic data provided below to determine ΔG (in kJ/mol) for the condensation of NaCl...
Use the thermodynamic data provided below to determine ΔG (in kJ/mol) for the condensation of NaCl at 138.08 °C if the initial partial pressure of NaCl is 1.62 atm. Report your answer to one decimal place in standard notation (i.e. 123.4 kJ/mol). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) NaCl (l) -385.9 95.1 NaCl (g) -181.4 229.8
Use the thermodynamic data provided below to determine ΔG (in kJ/mol) for the vaporization of CaO...
Use the thermodynamic data provided below to determine ΔG (in kJ/mol) for the vaporization of CaO at 91.8 °C if the initial partial pressure of CaO is 1.76 atm. Report your answer to one decimal place in standard notation (i.e. 123.4 kJ/mol). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) CaO (l) -557.3 62.3 CaO (g) 43.9 219.7
Use the thermodynamic data provided below to estimate the boiling point (in K) of ICl. Report...
Use the thermodynamic data provided below to estimate the boiling point (in K) of ICl. Report your answer to zero decimal places in standard notation (i.e. 123. kJ *For numbers ending in zero, be sure to include the decimal!*). Substance ΔH°f (kJ/mol) S° (J mol-1K-1) ICl (l) -23.89 135.1 ICl (g) 17.78 247.6
Use the thermodynamic data below to determine the equilibrium constant for the conversion of oxygen to...
Use the thermodynamic data below to determine the equilibrium constant for the conversion of oxygen to ozone at 3803°C 3O2 (g) ⇌ 2O3 (g) substance       ΔH˚f (kJ/mol)     ΔG˚f (kJ/mol)      S˚ (J/mol*K)        O2 (g) 0 0 205.0        O3 (g) 142.3 163.4                        237.6
Using a thermodynamic table below , determine the bond energy of F2, along with the fraction...
Using a thermodynamic table below , determine the bond energy of F2, along with the fraction of diatomics that have sufficient energy to react at 298K and 500K. ΔH°f (kJ mol-1) ΔG°f (kJ mol-1) S°m (J mol-1 K-1) Cp,m (J mol-1 K-1) Molecular weight F2(g) 0 0 202.8 31.3 38.00 F(g) 79.4 62.3 158.8 22.7 19.00
Standard enthalpies of formation are obtained from thermodynamic tables as: C2H5OH(l) -224 kJ/mol CO2(g) -398 kJ/mol...
Standard enthalpies of formation are obtained from thermodynamic tables as: C2H5OH(l) -224 kJ/mol CO2(g) -398 kJ/mol H2O(l) -281 kJ/mol. Calculate the enthalpy change of the reaction C2H5OH(l) + 3 O2 ? 2 CO2(g) + 3 H2O Follow the procedures based on Hess's Law: First write down the reactions corresponding to the enthalpies of formation you have been given, reverse the equations if necessary, remembering to change the sign of ?Ho, then combine the equations to give the required process, and...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l) (unbalanced) ΔHf C2H6 (g) = -84.7 kJ/mol; S C2H6 (g) = 229.5 J/K⋅mol; ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S CO2 (g) = 213.6 J/K⋅mol; ΔHf H2O (l) = -285.8 kJ/mol; SH2O (l) = 69.9 J/K⋅mol; SO2 (g) = 205.0 J/K⋅mol
Standard enthalpies of formation are obtained from thermodynamic tables as: C2H5OH(l) -227 kJ/mol CO2(g)    -390...
Standard enthalpies of formation are obtained from thermodynamic tables as: C2H5OH(l) -227 kJ/mol CO2(g)    -390 kJ/mol H2O(l)    -285 kJ/mol. Calculate the enthalpy change of the reaction C2H5OH(l) + 3 O2 ? 2 CO2(g) + 3 H2O Follow the procedures based on Hess's Law: First write down the reactions corresponding to the enthalpies of formation you have been given, reverse the equations if necessary, remembering to change the sign of ?Ho, then combine the equations to give the required...
Carbon disulfide (CS2) is a toxic, highly flammable substance. The following thermodynamic data are available for...
Carbon disulfide (CS2) is a toxic, highly flammable substance. The following thermodynamic data are available for CS2(l) and CS2(g) at 298 K: ΔH∘f (kJ/mol) ΔG∘f (kJ/mol) CS2(l) 89.7 65.3 CS2(g) 117.4 67.2 1. Liquid CS2 burns in O2 with a blue flame, forming CO2(g) and SO2(g). Write a balanced equation for this reaction. 2. Using the data in the preceding table and in Appendix C in the textbook, calculate ΔH∘ and ΔG∘ for the reaction in part D. 3. Use...
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF: ΔH°f (kJ/mol) IF7(g) +...
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF: ΔH°f (kJ/mol) IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ IF7(g) -941 IF5(g) -840 Answers: (a) -190 KJ/mol (b) 101 KJ/mol (c) 24 KJ/mol (d) -95 KJ/mol (e) -146 KJ/mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT