Question

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 corresponds to the temperature at which K < 1 changes to K > 1. Assume that ΔH° and ΔS° are constant and do not change with temperature. Fe3O4(s) + 4H2(g)3Fe(s) + 4H2O(g) ΔH° = 151 kJ/mol and ΔS° = 169 J/K ⋅ mol

T = ? K

Answer #1

kindly post different questions separately. please rate

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 14.50 mm Hg. N2(g) + 3H2(g)2NH3(g)

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...

1.
Calculate the standard free energy change at 500 K for the
following reaction.
Cu(s) +
H2O(g) à CuO(s) +
H2(g)
ΔH˚f
(kJ/mol)
S˚
(J/mol·K)
Cu(s)
0
33.3
H2O(g)
-241.8
188.7
CuO(s)
-155.2
43.5
H2(g)
0
130.6
2. When
solid ammonium nitrate dissolves in water, the resulting solution
becomes cold. Which is true and why?
a. ΔH˚
is positive and ΔS˚ is positive
b. ΔH˚
is positive and ΔS˚...

You are given the following thermodynamic data. 2 Fe(s) + 3/2
O2(g) → Fe2O3(s) ΔH° = -823 kJ 3 Fe(s) + 2 O2(g) → Fe3O4(s) ΔH° =
-1120. kJ Calculate the ΔH° for the following reaction. 3 Fe2O3(s)
→ 2 Fe3O4(s) + ½ O2(g)

Use standard free energies of formation to calculate ΔG∘ΔG∘ at
25 ∘C∘C for each of the following reactions.
Substance
ΔG∘f(kJ/mol)ΔGf∘(kJ/mol)
H2O(g)H2O(g)
−−228.6
H2O(l)H2O(l)
−−237.1
NH3(g)NH3(g)
−−16.4
NO(g)NO(g)
87.6
CO(g)CO(g)
−−137.2
CO2(g)CO2(g)
−−394.4
CH4(g)CH4(g)
−−50.5
C2H2(g)C2H2(g)
209.9
C2H6(g)C2H6(g)
−−32.0
Fe3O4(s)Fe3O4(s)
−−1015.4
KClO3(s)KClO3(s)
−−296.3
KCl(s)KCl(s)
−−408.5
Part A
C(s,graphite)+2H2(g)→CH4(g)C(s,graphite)+2H2(g)→CH4(g)
Express your answer to one decimal place and include the
appropriate units.
Part B
Fe3O4(s)+4H2(g)→3Fe(s)+4H2O(g)Fe3O4(s)+4H2(g)→3Fe(s)+4H2O(g)
Express your answer to one decimal place and include the
appropriate units.
Part C
N2(g)+O2(g)→2NO(g)N2(g)+O2(g)→2NO(g)
Express your answer...

Consider the reaction 2CO2(g) + 5H2(g)C2H2(g) + 4H2O(g) Using
the standard thermodynamic data in the tables linked above,
calculate G for this reaction at 298.15K if the pressure of each
gas is 17.64 mm Hg.
ANSWER:_____ kJ/mol

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...

Calculate the standard enthalpy of formation (∆H°f) at 298.15 K
for CO(g)
Known: Reaction ∆H°R298.15 K,
cal/mol for C(gr) + O2(g) →
CO2(g) = -94,052 cal/mol
and 2CO(g) + O2(g) → 2CO2(g) =
-135,272

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 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

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