Question

Use the thermodynamic data provided below to determine ΔG (in
kJ/mol) for the condensation of C_{2}H_{5}OH at
64.02 °C if the initial partial pressure of
C_{2}H_{5}OH 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^{-1}K^{-1}) |
||

C_{2}H_{5}OH (l) |
-277.7 | 160.7 | ||

C_{2}H_{5}OH (g) |
-235.1 | 282.7 |

Answer #1

For C2H5OH (l)

*G* = *H* - *TS*

*G* = -277.7 kJ/mol - 337.02
(0.1607kJ mol^{-1}K^{-1})

*G* = -331.85 kJ
mol^{-1}

For C2H5OH (g)

*G* = *H* - *TS*

*G* = -235.1 kJ
mol^{-1}- 337.02 (0.2827kJ
mol^{-1}K^{-1})

*G* = -330.375 kJ
mol^{-1}

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 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 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 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 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
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) + 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 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 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) + 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

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