Question

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^{-1}K^{-1}) |
||

CaO (l) | -557.3 | 62.3 | ||

CaO (g) | 43.9 | 219.7 |

Answer #1

For CaO (l)

*G* = *H* - *TS*

*G* = -557.3 kJ/mol - 364.95
(0.0623kJ mol^{-1}K^{-1})

*G* = -580.36 kJ
mol^{-1}

For CaO (l)

*G* = *H* - *TS*

*G* = 43.9 kJ
mol^{-1}- 364.95 (0.219.7kJ
mol^{-1}K^{-1})

*G* = 43.9 - 80.18

*G* = 36.28 kJ
mol^{-1}

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

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 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

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...

1) Given the following thermochemical reaction and thermodynamic
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N2(g) + 3H2(g) → 2NH3(g) ΔH = -91.8 kJ
ΔS[N2] = 191 J / mol · K, ΔS[H2] = 131 J / mol · K, and ΔS[NH3]
= 193 J / mol · K
a.98.3 kJ; Non-Spontaneous
b.-98.3 kJ; Spontaneous
c.32.7 kJ; Non-Spontaneous
d.ΔG = -32.7 kJ; Spontaneous
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delta Hfo (kJ/mol)
o (J/mol K
C(graphite)
0.0
5.740
C(diamond)
1.895
2.377
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