Question

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

NaCl (l) | -385.9 | 95.1 | ||

NaCl (g) | -181.4 | 229.8 |

Answer #1

Substance |
ΔH° |
S° (J mol |
||

NaCl (l) |
-385.9 |
95.1 |
||

NaCl (g) |
-181.4 |
229.8 |

NaCl(g) --> NaCl (l)

S = 229.8J mol^{-1}K^{-1} --> 95.1 J
mol^{-1}K^{-1}

dS = prod - reactant

dS =95.1 J mol^{-1}K^{-1}-229.8 J
mol^{-1}K^{-1}

= - 134.7 J mol^{-1}K^{-1}

=- 0.1347 kJ mol^{-1}K^{-1}

NaCl(g) --> NaCl (l)

H = -181.4KJ mol^{-1} --> -385.9K J
mol^{-1}

dH = prod - reactant

dH =-385.9 K J mol^{-1}-(-181.4) KJ mol^{-1}

dH = - 204.5 KJ mol^{-1}

138.08Celsius .... Kelvin temp = 411.23 K

dG = dH - TdS

dG = - 204.5 KJ mol^{-1}- ( 411.23K) (- 0.1347kJ/K
mol)

dG = - 204.5 KJ mol^{-1}+ 55.39 kJ / mol

**dG = - 259.89 kJ/mol or -259.9 kJ/mol**

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 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

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

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
data, find Gibbs Free Energy, ΔG, and determine if the reaction is
spontaneous or non-spontaneous at 25 °C?
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
2) What is the oxidation number...

Based on the thermodynamic properties provided for water,
determine the amount of energy released for 160.0 g of water to go
from 83.0 °C to -17.5 °C.
Property
Value
Units
Melting point
0.0
°C
Boiling point
100.0
°C
ΔHfusΔHfus
6.01
kJ/mol
ΔHvapΔHvap
40.67
kJ/mol
cp (s)
37.1
J/mol·°C
cp (l)
75.3
J/mol·°C
cp (g)
33.6
J/mol·°C

Based on the thermodynamic properties provided for water,
determine the amount of energy needed for 2.60 kg of water to go
from -4.00 °C to 74.0 °C.
Property
Value
Units
Melting point
0.0
°C
Boiling point
100.0
°C
ΔHfus
6.01
kJ/mol
ΔHvap
40.67
kJ/mol
cp (s)
37.1
J/mol ·°C
cp (l)
75.3
J/mol ·°C
cp (g)
33.6
J/mol ·°C

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