Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 102 M to 2.5 x 10²M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. T' T. O Word(s) III !!!

Use this information to answer Questions 3, 4, and 5: The equilibrium constant (K) of the reaction below is K = 6.0 x 10-2, with initial concentrations as follows: [H2] = 1.0 x 102 M, [N2] = 4.0 M, and [NH3] = 1.0 x 104M. N2(g) + 3H2(g) = 2NH3(g) 3. Consider the chemical reaction: N2 + 3H2yields 2NH3. If the concentration of the reactant H2 was increased from 1.0 x 102 M to 2.5 x 10²M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. T' T. O Word(s) III !!!

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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