?The value of the equilibrium constant \(K_{c}\) for the reaction \(\mathrm{N}_{2}(g)+3

Chapter 15, Problem 15.75

(choose chapter or problem)

The value of the equilibrium constant \(K_{c}\) for the reaction \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)\) changes in the following manner as a function of temperature

(a) Based on the changes in \(K_{c}\) is this reaction exothermic or endothermic?

(b) Use the standard enthalpies of formation given in Appendix C to determine the \(\Delta H\) for this reaction at standard conditions. Does this value agree with your prediction from part (a)?

(c) If 0.025 mole of gaseous \(\mathrm{NH}_{3}\) is added to a 1.00 L container and heated to \(500^{\circ} \mathrm{C}\), what is the concentration of \(\mathrm{NH}_{3}\) once the sample reaches equilibrium?

Text Transcription:

K_c

N_2(g)+3 H_2(g) rightleftharpoons 2 NH_3(g)

Delta H

NH_3

500^circ C