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

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 27P

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