Nitrogen dioxide undergoes a reversible dimerization reaction according to the following equation: 2NO2 = N2O4 If 0.2 mole NO2 is placed in a 1.0 L flask at 298K and the reaction is allowed to reach equilibrium, one finds that at equilibrium, the flask contains 0.0204 mole NO2 and 0.0898 mole N2O4. From this information find both the concentration-based equilibrium constant (Kc) and the pressure-based equilibrium constant (Kp)
Nitrogen dioxide undergoes a reversible dimerization reaction according to the following equation: 2NO2 = N2O4 If 0.2 mole NO2 is placed in a 1.0 L flask at 298K and the reaction is allowed to reach equilibrium, one finds that at equilibrium, the flask contains 0.0204 mole NO2 and 0.0898 mole N2O4. From this information find both the concentration-based equilibrium constant (Kc) and the pressure-based equilibrium constant (Kp)
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...
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- Nitrogen dioxide undergoes a reversible dimerization reaction according to the following equation:
2NO2 = N2O4 If 0.2 mole NO2 is placed in a 1.0 L flask at 298K and the reaction is allowed to reach equilibrium, one finds that at equilibrium, the flask contains 0.0204 mole NO2 and 0.0898 mole N2O4. From this information find both the concentration-based equilibrium constant (Kc) and the pressure-based equilibrium constant (Kp).
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