Consider the following equilibrium reaction: N2O4 (g) 2 NO₂ (g) A 2.000-L flask is initially filled with 6.00 X10^-2 mol of N204. At equilibrium, 2.36X10^-2 mol/L of N2O4 remains in the flask. Find the equilibrium constant.

Consider the following equilibrium reaction: N2O4 (g) 2 NO₂ (g) A 2.000-L flask is initially filled with 6.00 X10^-2 mol of N204. At equilibrium, 2.36X10^-2 mol/L of N2O4 remains in the flask. Find the equilibrium constant.

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.50E

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Question

C
Consider the following equilibrium reaction:
N₂O4 (g) 2 NO2 (g)
A 2.000-L flask is initially filled with 6.00 X10^-2 mol of N204. At equilibrium,
2.36X10^-2 mol/L of N204 remains in the flask.
Find the equilibrium constant.
1.92 x10^-4
6.94 x10^-3
0.391
0.212
0.723
C
yang

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