Chemistry 146
Part A
What is the equilibrium constant of the reaction at 25°C if ΔG° = -50.5 kJ?
C(s, graphite) + 2 H2(g) ⇌ CH4(g)
7.1×108
10-50.5
1.0
20 2. Part A
Calculate the ΔG°rxn using the following information.
2HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l)
ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K)
ΔG°rxn = ? 210.8 240.1 70.0 46.0 +50.8 kJ
-85.5 kJ
-151 kJ
-186 kJ
+222 kJ 3. Part A
Determine ΔG°rxn using the following information.
FeO(s) + CO(g) → Fe(s) + CO2(g) ΔH°= -11.0 kJ; ΔS°= -17.4 J/K
+1.6 kJ
+191.0 kJ
+89.5 kJ
-6.4 kJ -5.8 kJ 4. Part A
Calculate the ΔG°rxn using the following information.
2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g)
ΔH°f(kJ/mol) -20.6
S°(J/mol∙K)
ΔG°rxn = ? 205.8 205. 296.8 -241.8 248.2 188.8 +108.2 kJ
-466.1 kJ
+196.8 kJ
+676.2 kJ
-147.1 kJ 5. Part A
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction.
SO3(g) + H2O(g) → H2SO4(l) ΔG°= -90.5 kJ
P(SO3) = 0.20 atm, P(H2O) = 0.88 atm -30.4 kJ
+15.9 kJ
+51.4 kJ
-86.2 kJ
-90.5 kJ 6. Part A
Which one of the following would be expected to have the lowest standard molar entropy, S°, at
25°C?
C 14 H 30 ( s )
C 10 H 22 ( s )
C 10 H 22 ( l ) C 14 H 30 OH( l 7. Part A
Which of the following processes have a ΔS < 0?
water freezes
methanol (g, at 555 K) → methanol (g, at 400 K)
carbon dioxide(g) → carbon dioxide(s)
isopropyl alcohol condenses
All of the above processes have a ΔS < 0. 8. Part A
Place the following in order of increasing molar entropy at 298 K.
NO CO SO
SO < NO < CO
CO < SO < NO
SO < CO < NO
NO < CO < SO
CO < NO < SO 9. art A
Determine the equilibrium constant for the following reaction at 549 K.
CH2O(g) + 2 H2(g) → CH4(g) + H2O(g) ΔH° = -94.9 kJ; ΔS°= -224.2 J/K
2.08 x 10-3
1.07 x 109
481
1.94 x 10-12
9.35 x 10-10 10. Part A Calculate ΔS°rxn for the following reaction. The S° for each species is shown below the reaction.
N2H4(l) + H2(g) → 2 NH3(g)
S° (J/mol∙K) 121.2 130.7 192.8 -202.3 J/K
+133.7 J/K
+178.9 J/K
-59.1 J/K
+118.2 J/K 11. Part A
Determine the equilibrium constant for the following reaction at 655 K.
HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K
2.51 × 10-13
13.0
3.07 × 1011
3.99 × 1012
3.26 × 10-12 12. Part A
Which of the following processes shows a decrease in entropy of the system?
2 NO(g) + O2(g) → 2 NO2(g)
CH3OH(l) → CO(g) + 2H2(g)
COCl2(g) → CO(g) + Cl2(g)
NaClO3(s) →Na+(aq) + ClO3-(aq)
None of the above will show a decrease in entropy. 13. Part A
Determine ΔG°rxn using the following information. CaCO3(s) → CaO(s) + CO2(g) ΔH°= +179.2 kJ; ΔS°= +160.2 J/K
+228.1 kJ
-89.3 kJ
+112 .0 kJ
+131.4 kJ
-607.0 kJ 14. Part A
Place the following in order of decreasing molar entropy at 298 K.
H2 Cl2 F2
F2 > Cl2 > H2
Cl2 > H2 > F2
Cl2 > F2 > H2
H2 > F2 > Cl2
H2 > Cl2 > F2 15. Part A
Calculate the ΔG°rxn using the following information.
2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ?
ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
-54.5 kJ
-162.5 kJ
+171.1 kJ
-87.6 kJ
+51.0 kJ 16. Part A
Estimate ΔG°rxn for the following reaction at 775 K. 2 Hg(g) + O2(g) → 2 HgO(s) ΔH°= -304.2 kJ; ΔS°= -414.2 J/K
+17 kJ
-181 kJ
+321 kJ
-625 kJ
-110 kJ 17. Part A
Determine the equilibrium constant for the following reaction at 298 K.
SO3(g) + H2O(g) → H2SO4(l) ΔG° = -90.5 kJ
7.31 × 1015
0.964
1.37 × 10-16
9.11 × 10-8
4.78 × 1011
18. A reaction has an equilibrium constant of Kp=0.231 at 32 ∘C. 19. Part A
Which of the following processes have a ΔS > 0?
CH4(g) + H2O(g) → CO(g) + 3 H2(g)
CH3OH(l) → CH3OH(s)
N2(g) + 3 H2(g) → 2 NH3(g)
Na2CO3(s) + H2O(g) + CO2(g) → 2 NaHCO3(s)
All of the above processes have a ΔS > 0. 20. Part A
Above what temperature does the following reaction become
nonspontaneous?
2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH = -1036 kJ; ΔS =
-153.2 J/K

 

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