**Equilibrium Constant Calculation****The equilibrium constant, Kc, for the following reaction is 5.32 at 716 K:**\[ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) \]**Calculate Kc at this temperature for the following reaction:**\[ \text{NH}_3(g) \rightleftharpoons \frac{1}{2}\text{N}_2(g) + \frac{3}{2}\text{H}_2(g) \]\[ K_c = \]The equilibrium constant (Kc) for the reaction \[ \text{NH}_3(g) \rightleftharpoons \frac{1}{2}\text{N}_2(g) + \frac{3}{2}\text{H}_2(g) \]can be derived from the given reaction \[ 2\text{NH}_3(g) \rightleftharpoons \text{N}_2(g) + 3\text{H}_2(g) \]Since the second reaction is exactly one-half of the first reaction, the equilibrium constant for the second reaction can be calculated using the relationship:\[ K'_{c} = (K_{c})^{1/n} \]where \( n \) is the factor by which the original reaction is multiplied (or divided, in this case, n = 2).Therefore:\[ K'_{c} = (5.32)^{1/2} \]Perform the calculation to obtain the value of \( K'_{c} \).

In this question, we want to determine the new Equilibrium constant ( Kc ) for second Reaction. You…

Answered: The equilibrium constant, K., for the…

The equilibrium constant, K., for the following reaction is 5.32 at 716 K. 2NH3(g) N2(g) + 3H2(g) Calculate K, at this temperature for the following reaction: NH3(g) 1/2N2(g) + 3/2H2(g) K = |

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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