Question

Use the thermodynamic data below to determine the equilibrium
constant for the conversion of oxygen to ozone at 3803°C

3O_{2 (}_{g}_{)} ⇌ 2O_{3
(}_{g}_{)}

**substance Δ H˚f
(kJ/mol) ΔG˚f
(kJ/mol) S˚ (J/mol*K)**

O_{2
(}_{g}_{)} 0 0 205.0

O_{3
(}_{g}_{)} 142.3
163.4
237.6

Answer #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 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 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

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

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

1)Use standard thermodynamic data (in the Chemistry References)
to calculate G at 298.15 K for the following reaction, assuming
that all gases have a pressure of 19.31 mm Hg. 2N2(g) +
O2(g)2N2O(g)
G = ? kJ/mol
2)Using standard thermodynamic data (linked), calculate the
equilibrium constant at 298.15 K for the following reaction.
C2H4(g) + H2O(g)CH3CH2OH(g)
K = ?
3) Calculate the temperature (in kelvins) at which the sign of
G° changes from positive to negative for the reaction below. This...

Use the free energies of formation given below to calculate the
equilibrium constant (K) for the following reaction at 298 K.
2 HNO3(aq) + NO(g) → 3 NO2(g) +
H2O(l) K = ?
ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
Calculate the ΔG∘rxn for the reaction using the following
information.
4HNO3(g)+5N2H4(l)→7N2(g)+12H2O(l)
ΔG∘f(HNO3(g)) = -73.5 kJ/mol;
ΔG∘f(N2H4(l)) = 149.3 kJ/mol;
ΔG∘f(N2(g)) = 0 kJ/mol;
ΔG∘f(H2O(l)) = -273.1 kJ/mol.
Calculate the ΔG°rxn using the following
information.
2 H2S(g) + 3 O2(g) → 2...

he thermodynamic properties for a reaction are related by the
equation that defines the standard free energy, ΔG∘, in
kJ/mol:
ΔG∘=ΔH∘−TΔS∘
where ΔH∘ is the standard enthalpy change in kJ/mol and
ΔS∘ is the standard entropy change in J/(mol⋅K). A good
approximation of the free energy change at other temperatures,
ΔGT, can also be obtained by utilizing this
equation and assuming enthalpy (ΔH∘) and entropy
(ΔS∘) change little with temperature.
Part A
For the reaction of oxygen and nitrogen to...

The element oxygen was prepared by Joseph Priestley in 1774 by
heating mercury (II) oxide.
HgO(s) --> Hg(l) + 1/2O2(g) ΔH° = 90.84 kJ
Use the data given below to determine DS
= and the temperature, at which this
reaction will become spontaneous under standard conditions.
S°(Hg) = 76.02 J/K· mol
S°(O2) = 205.0 J/K· mol
S°(HgO) = 70.29 J/K· mol

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...

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