Part A A sample of pure NO2 is heated to 334 °C at which temperature it partially dissociates according to the equation 2 NO2 (g) = 2 NO (g) + O2 (9) At equilibrium the density of the gas mixture is 0.520 g/L at 0.750 atm . Calculate K. for the reaction.

Part A A sample of pure NO2 is heated to 334 °C at which temperature it partially dissociates according to the equation 2 NO2 (g) = 2 NO (g) + O2 (9) At equilibrium the density of the gas mixture is 0.520 g/L at 0.750 atm . Calculate K. for the reaction.

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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Question

Part A
A sample of pure NO2 is heated to 334 °C at which
temperature it partially dissociates according to the
equation
2 NO2 (g) = 2 NO (g) + O2 (g)
At equilibrium the density of the gas mixture is 0.520
g/L at 0.750 atm .
Calculate K. for the reaction.
Π ΑΣφ.
K = .0133
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