4. The equilibrium constant (Kp) for the following reaction is 0.113 at 298 K, which corresponds to a standard free-energy change of 5.40 kJ/mol. In a certain experiment, the initial pressures are PNO2 = 0.122 atm and PN204 = 0.453 atm. Calculate AG for the reaction at these pressures and predict the direction of the net reaction at equilibrium, take the gas constant (R) value as 8.314 J/K.mol. N204(g) → 2NO2(g)
4. The equilibrium constant (Kp) for the following reaction is 0.113 at 298 K, which corresponds to a standard free-energy change of 5.40 kJ/mol. In a certain experiment, the initial pressures are PNO2 = 0.122 atm and PN204 = 0.453 atm. Calculate AG for the reaction at these pressures and predict the direction of the net reaction at equilibrium, take the gas constant (R) value as 8.314 J/K.mol. N204(g) → 2NO2(g)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Can you please solve number 4 and show all of the steps to the solution
![### Problem 4:
The equilibrium constant (\(K_p\)) for the following reaction is 0.113 at 298 K, which corresponds to a standard free-energy change of 5.40 kJ/mol. In a certain experiment, the initial pressures are \(P_{NO_2} = 0.112 \, \text{atm}\) and \(P_{N_2O_4} = 0.453 \, \text{atm}\). Calculate \(\Delta G\) for the reaction at these pressures and predict the direction of the net reaction at equilibrium. Take the gas constant (\(R\)) value as 8.314 J/K·mol.
\[ N_2O_4(g) \rightarrow 2 NO_2(g) \]
### Problem 5:
Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral.
| Compound | Solution is... |
|----------|----------------|
| CCl\(_3\) | ⬤ neutral |
| NH\(_4\)Br | ⬤ acidic |
Each compound is evaluated to determine whether it forms an acidic, basic, or neutral solution when dissolved in water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e830786-058e-49dd-8798-047547f22476%2F2258638c-3417-45bb-b207-43b10b1af3f6%2Ffiuudjm.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem 4:
The equilibrium constant (\(K_p\)) for the following reaction is 0.113 at 298 K, which corresponds to a standard free-energy change of 5.40 kJ/mol. In a certain experiment, the initial pressures are \(P_{NO_2} = 0.112 \, \text{atm}\) and \(P_{N_2O_4} = 0.453 \, \text{atm}\). Calculate \(\Delta G\) for the reaction at these pressures and predict the direction of the net reaction at equilibrium. Take the gas constant (\(R\)) value as 8.314 J/K·mol.
\[ N_2O_4(g) \rightarrow 2 NO_2(g) \]
### Problem 5:
Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral.
| Compound | Solution is... |
|----------|----------------|
| CCl\(_3\) | ⬤ neutral |
| NH\(_4\)Br | ⬤ acidic |
Each compound is evaluated to determine whether it forms an acidic, basic, or neutral solution when dissolved in water.
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