General Chemistry 2: Thermodynamics and Equilibrium
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N##_2## (g) + 3 H##_2## (g) ##\leftrightharpoons## 2 NH##_3## (g)
For the reaction above what is ##\triangle##H##^\circ## given that ##\triangle##H##_f^\circ## for NH##_3## (g) is -45.9 kJ/mol at 25##^\circ##C?
For the reaction above what is ##\triangle##H##^\circ## given that ##\triangle##H##_f^\circ## for NH##_3## (g) is -45.9 kJ/mol at 25##^\circ##C?
N##_2## (g) + 3 H##_2## (g) ##\leftrightharpoons## 2 NH##_3## (g)
For the reaction above, what is the sign and value of entropy for the reaction, given:
H##_2## (g), S##^\circ##(at 25##^\circ##C) = 130.7 J/(mol*K)
N##_2## (g), S##^\circ##(at 25##^\circ##C) = 191.56 J/(mol*K)
NH##_3## (g), S##^\circ##(at 25##^\circ##C) = 192.77 J/(mol*K)
For the reaction above, what is the sign and value of entropy for the reaction, given:
H##_2## (g), S##^\circ##(at 25##^\circ##C) = 130.7 J/(mol*K)
N##_2## (g), S##^\circ##(at 25##^\circ##C) = 191.56 J/(mol*K)
NH##_3## (g), S##^\circ##(at 25##^\circ##C) = 192.77 J/(mol*K)
N##_2## (g) + 3 H##_2## (g) ##\leftrightharpoons## 2 NH##_3## (g)
For the reaction above, calculate the change in free energy for the reaction, if it were to go to completion.
For the reaction above, calculate the change in free energy for the reaction, if it were to go to completion.
N##_2## (g) + 3 H##_2## (g) ##\leftrightharpoons## 2 NH##_3## (g)
For the reaction above, calculate the free energy of formation, ##\triangle##G##_f^\circ## for each of the products and reactions.
For the reaction above, calculate the free energy of formation, ##\triangle##G##_f^\circ## for each of the products and reactions.
Calculate the standard free energy change, ##\triangle##G##^\circ##, for the following reaction. Is the reaction spontaneous?
CH##_4## (g) + 2 O##_2## (g) ##\longrightarrow## CO##_2## (g) + 2 H##_2##O (l)
Values of standard molar entropy, S##_{f}^\circ## are as follows: CH##_4## (g), 186 J/(K*mol); O##_2## (g), 205 J/(K*mol); CO##_2## (g), 213.6 J/(K*mol); 2 H##_2##O (l), 69.9 J/(K*mol)
##\triangle##H##^\circ## for this reaction is -890.3 kJ
CH##_4## (g) + 2 O##_2## (g) ##\longrightarrow## CO##_2## (g) + 2 H##_2##O (l)
Values of standard molar entropy, S##_{f}^\circ## are as follows: CH##_4## (g), 186 J/(K*mol); O##_2## (g), 205 J/(K*mol); CO##_2## (g), 213.6 J/(K*mol); 2 H##_2##O (l), 69.9 J/(K*mol)
##\triangle##H##^\circ## for this reaction is -890.3 kJ
What is the standard free energy change, ##\triangle##G##^\circ##, for the following reaction at 298 K? Is the reaction spontaneous?
2 PCl##_3## (g) + O##_2## (g) ##\longrightarrow## 2 POCl##_3##, ##\triangle##H = - 620.6 kJ/mol
Values of standard molar entropy, S##_{f}^\circ## are as follows: 2 PCl##_3## (g), 311.8 J/K; O##_2## (g), 205.1 J/K; POCl##_3##, 222.4 J/K
2 PCl##_3## (g) + O##_2## (g) ##\longrightarrow## 2 POCl##_3##, ##\triangle##H = - 620.6 kJ/mol
Values of standard molar entropy, S##_{f}^\circ## are as follows: 2 PCl##_3## (g), 311.8 J/K; O##_2## (g), 205.1 J/K; POCl##_3##, 222.4 J/K
What is the standard free energy change, ##\triangle##G##^\circ##, for the following reaction?
Zn (s) + 2 H##^+## (aq) ##\longrightarrow## Zn##^{2+}## (aq) + H##_2## (g), 25##^\circ##C
Standard free energies of formation, ##\triangle##G##_{f}^\circ## are as follows: Zn (s), 0 kJ/mol; 2 H##^+## (aq), 0 kJ/mol; Zn##^{2+}## (aq), -147.1 kJ/mol; H##_2## (g), 0 kJ/mol
Zn (s) + 2 H##^+## (aq) ##\longrightarrow## Zn##^{2+}## (aq) + H##_2## (g), 25##^\circ##C
Standard free energies of formation, ##\triangle##G##_{f}^\circ## are as follows: Zn (s), 0 kJ/mol; 2 H##^+## (aq), 0 kJ/mol; Zn##^{2+}## (aq), -147.1 kJ/mol; H##_2## (g), 0 kJ/mol