1. The Ka for acetic acid is 1.80 x 10-5. What is the value of AG°xn for the ionization of acetic acid in water at 25 °C? (27.1 kJ) 2. The AG° for a gas-phase reaction is +6.7 kJ. Calculate the value of Kp at 298K. (0.067) 3. Use the equation and]values below for the next 3 questions. 2N2O(g) + 302(g) 110 4NO2(g) AH-31.6 kJ AS°=-98.0 J/K a. Calculate AG°, in kJ, for the reaction at 298 K. (2.4 kJ) b. Calculate the equilibrium constant at 425 K for this reaction. (0.058) c. When 1.00 M NO2 (g), 0.50 M O2 (g) and 0.50 M N2O are mixed in a container at 298 K, which of the substance(s) will increase in concentration? (left) d. Use a completely different strategy to find the answer to part c. 4. If a 0.115 M solution of a weak acid, HX, has a pH of 4.973 at 25 °C, what is AG°, in kJ, for the dissociation reaction of this acid at 25 °C? (51.4 kJ) 5. What is the pH of a 0.198 M solution of a weak base B if AH° = -22.3 kJ and AS° = -164 J/K for the following equilibrium at 25 °C? (pH = 11.32) B(aq) + H2O(1) 12 BH(aq) + OH(aq)
1. The Ka for acetic acid is 1.80 x 10-5. What is the value of AG°xn for the ionization of acetic acid in water at 25 °C? (27.1 kJ) 2. The AG° for a gas-phase reaction is +6.7 kJ. Calculate the value of Kp at 298K. (0.067) 3. Use the equation and]values below for the next 3 questions. 2N2O(g) + 302(g) 110 4NO2(g) AH-31.6 kJ AS°=-98.0 J/K a. Calculate AG°, in kJ, for the reaction at 298 K. (2.4 kJ) b. Calculate the equilibrium constant at 425 K for this reaction. (0.058) c. When 1.00 M NO2 (g), 0.50 M O2 (g) and 0.50 M N2O are mixed in a container at 298 K, which of the substance(s) will increase in concentration? (left) d. Use a completely different strategy to find the answer to part c. 4. If a 0.115 M solution of a weak acid, HX, has a pH of 4.973 at 25 °C, what is AG°, in kJ, for the dissociation reaction of this acid at 25 °C? (51.4 kJ) 5. What is the pH of a 0.198 M solution of a weak base B if AH° = -22.3 kJ and AS° = -164 J/K for the following equilibrium at 25 °C? (pH = 11.32) B(aq) + H2O(1) 12 BH(aq) + OH(aq)
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
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Help solve 1,2,3,4,5.
![1. The Ka for acetic acid is 1.80 x 10-5. What is the value of AG°xn for the ionization of
acetic acid in water at 25 °C? (27.1 kJ)
2. The AG° for a gas-phase reaction is +6.7 kJ. Calculate the value of Kp at 298K. (0.067)
3. Use the equation and]values below for the next 3 questions.
2N2O(g) + 302(g)
110
4NO2(g)
AH-31.6 kJ AS°=-98.0 J/K
a. Calculate AG°, in kJ, for the reaction at 298 K. (2.4 kJ)
b. Calculate the equilibrium constant at 425 K for this reaction. (0.058)
c. When 1.00 M NO2 (g), 0.50 M O2 (g) and 0.50 M N2O are mixed in a container at
298 K, which of the substance(s) will increase in concentration? (left)
d. Use a completely different strategy to find the answer to part c.
4. If a 0.115 M solution of a weak acid, HX, has a pH of 4.973 at 25 °C, what is AG°, in kJ,
for the dissociation reaction of this acid at 25 °C? (51.4 kJ)
5. What is the pH of a 0.198 M solution of a weak base B if AH° = -22.3 kJ and AS° =
-164 J/K for the following equilibrium at 25 °C? (pH = 11.32)
B(aq) + H2O(1)
12
BH(aq) + OH(aq)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5cec0502-895c-4b17-8c29-34d928502e7c%2F9166c9b9-50b9-4b0b-93c3-788cb8313f9b%2Fbrog0qp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. The Ka for acetic acid is 1.80 x 10-5. What is the value of AG°xn for the ionization of
acetic acid in water at 25 °C? (27.1 kJ)
2. The AG° for a gas-phase reaction is +6.7 kJ. Calculate the value of Kp at 298K. (0.067)
3. Use the equation and]values below for the next 3 questions.
2N2O(g) + 302(g)
110
4NO2(g)
AH-31.6 kJ AS°=-98.0 J/K
a. Calculate AG°, in kJ, for the reaction at 298 K. (2.4 kJ)
b. Calculate the equilibrium constant at 425 K for this reaction. (0.058)
c. When 1.00 M NO2 (g), 0.50 M O2 (g) and 0.50 M N2O are mixed in a container at
298 K, which of the substance(s) will increase in concentration? (left)
d. Use a completely different strategy to find the answer to part c.
4. If a 0.115 M solution of a weak acid, HX, has a pH of 4.973 at 25 °C, what is AG°, in kJ,
for the dissociation reaction of this acid at 25 °C? (51.4 kJ)
5. What is the pH of a 0.198 M solution of a weak base B if AH° = -22.3 kJ and AS° =
-164 J/K for the following equilibrium at 25 °C? (pH = 11.32)
B(aq) + H2O(1)
12
BH(aq) + OH(aq)
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