At a certain temperature, Kp = 0.23 for the reaction: N₂O4 (g) 2 NO₂ (g) At equilibrium, the pressure of N₂O4 (g) is 3.37 atm and the pressure of NO₂ (g) is 0.874 atm. The volume of the container is decreased to one-half of the original volume, and the temperature is held constant. Calculate the new equilibrium pressure of NO2 (g) In atm. Do NOT include units in your answer. If you round during your calculation, be sure to keep at least four (4) decimal places. Report your final answer to two (2) decimal places. Answer: 1.51 X

At a certain temperature, Kp = 0.23 for the reaction: N₂O4 (g) 2 NO₂ (g) At equilibrium, the pressure of N₂O4 (g) is 3.37 atm and the pressure of NO₂ (g) is 0.874 atm. The volume of the container is decreased to one-half of the original volume, and the temperature is held constant. Calculate the new equilibrium pressure of NO2 (g) In atm. Do NOT include units in your answer. If you round during your calculation, be sure to keep at least four (4) decimal places. Report your final answer to two (2) decimal places. Answer: 1.51 X

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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