4. Consider the decomposition of nitrogen trifluoride into nitrogen and fluorine below: 2 NF3 5 N2(9) + 3 F2(g) a) When 2.06 mol of NF, is initially placed in a 2.00 L container and allowed to come to equilibrium at 800K, the equilibrium mixture is found to contain 0.0228 mol of N2 gas. What is the equilibrium constant at this temperature? (1K/U, 1T/I, 1A) b) After decreasing the temperature, the equilibrium constant changes to Keg = 4.5 x 106 the concentrations become the following: [NF] = 1.00 M, [F] = 0.042 M and [N,] = 0.014 M, %3D i. Determine the reaction quotient, Q (2A) ii. Is the system at equilibrium? If it is not, describe how the system has to shift in order to reach equilibrium. (1C) E Tabl e

4. Consider the decomposition of nitrogen trifluoride into nitrogen and fluorine below: 2 NF3 5 N2(9) + 3 F2(g) a) When 2.06 mol of NF, is initially placed in a 2.00 L container and allowed to come to equilibrium at 800K, the equilibrium mixture is found to contain 0.0228 mol of N2 gas. What is the equilibrium constant at this temperature? (1K/U, 1T/I, 1A) b) After decreasing the temperature, the equilibrium constant changes to Keg = 4.5 x 106 the concentrations become the following: [NF] = 1.00 M, [F] = 0.042 M and [N,] = 0.014 M, %3D i. Determine the reaction quotient, Q (2A) ii. Is the system at equilibrium? If it is not, describe how the system has to shift in order to reach equilibrium. (1C) E Tabl e

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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