Consider the chemical reaction: N₂ + 3H2 yields 2NH3. If the concentration of the reactant H₂ was increased from 1.0 x 10-2 M to 2.5 x 10-¹ M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. 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 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N₂(g) + 3H₂(g) = 2NH3 (g)

Consider the chemical reaction: N₂ + 3H2 yields 2NH3. If the concentration of the reactant H₂ was increased from 1.0 x 10-2 M to 2.5 x 10-¹ M, calculate the reaction quotient (Q) and determine which way the chemical system would shift by comparing the value of Q to K. 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 10-2 M, [N₂] = 4.0 M, and [NH3] = 1.0 x 10-4 M. N₂(g) + 3H₂(g) = 2NH3 (g)

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 86QRT

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