Question
Use the free energies of formation given below to calculate the equilibrium constant (K) for the...
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 SO2(g) + 2
H2O(g) ΔG°rxn = ?
ΔG°f (kJ/mol) -33.4 -3300.1 -228.6
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19) Use the free energies of formation given below to calculate the equilibrium constant (K) for...
19) 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))...
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 for the reaction using the following
information.
= -73.5 ;
= 149.3 ;
= 0 ;
= -273.1 .
-312.9 kJ
+110.7 kJ
-954.7 kJ
-3.298 x 103 kJ
+2.845 x 103 kJ
Use standard free energies of formation to calculate ΔG∘ΔG∘ at 25 ∘C∘C for each of the...
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...
1.Using the enthalpies of formation given below, calculate ΔH°rxn in kJ, for the following reaction. Report...
1.Using the enthalpies of formation given below, calculate
ΔH°rxn in kJ, for the following reaction.
Report your answer to two decimal places in standard
notation.
H2S(g) + 2O2(g) → SO3(g) +
H2O(l)
H2S (g): -20.60 kJ/mol
O2 (g): 0.00 kJ/mol
SO3 (g): -395.77 kJ/mol
H2O (l): -285.83 kJ/mol
2. Calculate the amount of heat absorbed/released (in kJ) when
22.54 grams of SO3 are produced via the above
reaction.
Report your answer to two decimal places, and use appropriate signs
to...
Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following...
Use standard free energies of formation to calculate ΔG∘ at 25∘C
for each of the following reactions.
N2O4(g)→2NO2(g)
ΔG∘rxn =
2.8
kJ
NH4Cl(s)→HCl(g)+NH3(g)
ΔG∘rxn =
91.2
kJ
3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g)
ΔG∘rxn =
56.4
kJ
N2(g)+3H2(g)→2NH3(g)
ΔG∘rxn = -32.8 kJ
How do the values of ΔG∘ calculated this way compare to those
calculated from ΔH∘ and ΔS∘? Which of the two methods could be used
to determine how ΔG∘ changes with temperature? Essay answers are
limited to about 500 words (3800 characters maximum,...
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation...
9. Use the following experimentally derived combustion
data to calculate the standard molar enthalpy of formation
(ΔH°f ) of liquid methanol (CH3OH) from its
elements.
2 CH3OH(l) + 3 O2(g) → 2
CO2(g) + 4 H2O(l)
ΔH°rxn = −1452.8 kJ
C(graphite) + O2(g) →
CO2(g)
ΔH°rxn = −393.5 kJ
2 H2(g) + O2(g) → 2
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ΔH°rxn = −571.6 kJ
(1) −238.7 kJ/mol (2) 487.7
kJ/mol (3) −548.3 kJ/mol
(4) 20.1 kJ/mol
(5) 47.1 kJ/mol
Given the following information below, use Hess’s Law to calculate the enthalpy of formation for sodium...
Given the following information below, use Hess’s Law to
calculate the enthalpy of formation for sodium oxide:
Na (s) +
HCl (l) à NaCl (aq) + ½ H2
(g)
∆HRx
= -393.1 kJ/mol
Na2O (s)
+ 2 HCl (l) à 2 NaCl
(aq) + H2O
∆HRx
= -675.2 kJ/mol
H2 (g)
+ ½ O2
(g) à H2O
(g) ∆HRx
= -288.1 kJ/mol
2 Na (s)
+ ½ O2
(g) à Na2O
(s)
∆HRx
= __________ kJ/mol
Calculated Heat of Reaction is....?
(Put your answer in...
A. Using given data, calculate the change in Gibbs free energy for each of the following...
A. Using given data, calculate the change in
Gibbs free energy for each of the following reactions. In each case
indicate whether the reaction is spontaneous at 298K under standard
conditions.
2H2O2(l)→2H2O(l)+O2(g)
Gibbs free energy for H2O2(l) is -120.4kJ/mol
Gibbs free energy for H2O(l) is -237.13kJ/mol
B. A certain reaction has ΔH∘ = + 35.4
kJ and ΔS∘ = 85.0 J/K . Calculate ΔG∘ for the
reaction at 298 K. Is the reaction spontaneous at
298K under standard
conditions?
a) Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ...
a) Calculate the equilibrium constant at 17 K for a reaction
with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round until the
end. Using the exponent enlarges any round-off error.)
b) Calculate the equilibrium constant at 146 K for the
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larger at the larger temperature for an endothermic reaction)
c) Calculate the equilibrium constant at 43 K for a reaction
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ΔSrxno...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
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;
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