The standard free energy of formation of ammonia is \( -16.5 \, \text{kJ/mol} \).\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]**1st attempt**What is the value of \( K \) for the reaction below at 485.0 K? \[ \_\_\_\_\_\_\_\_\_\_\_ \]This text is part of an educational exercise that requires calculating the equilibrium constant (\( K \)) for the synthesis of ammonia from nitrogen and hydrogen gases at a specified temperature. The reaction is given as:\[ \text{N}_2 (g) + 3\text{H}_2 (g) \rightleftharpoons 2\text{NH}_3 (g) \]The standard free energy change for the formation of ammonia is provided, and the task involves determining the equilibrium constant at a specific temperature.

The reaction given is, => N2 (g) + 3 H2 (g) ------> 2 NH3 (g) Given : ΔGo = -16.5 KJ/mol = -16500 J/mol (since 1 KJ = 1000 J) The relationship between the ΔG0 and equilibrium constant is given by => RTln(K) = -ΔG0 where R = gas constant = 8.314 J/K.mol T = Temperature in Kelvin = 485.0 K K = equilibrium constant Hence substituting the values we get, => 8.314 X 485.0 X ln(K) = -(-16500 ) => ln(K) = 4.092 approx. => K = equilibrium constant = e4.092 = 59.86 approx.

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The standard free energy of formation of ammonia is - 16.5 kJ/mol. N, (g) + 3H,(g) – 2NH, (g) v 1st attempt What is the value of K for the reaction below at 485.0K?

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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