?Consider the reaction\(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \rightleftharpoons

Chapter 15, Problem 15.62

(choose chapter or problem)

Consider the reaction

\(4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) & \rightleftharpoons \\

4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(g), \Delta H=-904.4 \mathrm{~kJ}\)

Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium?

(a) increase \(\left[\mathrm{NH}_{3}\right]\) ;

(b) increase \(\left[\mathrm{H}_{2} \mathrm{O}\right]\) ;

(c) decrease \(\left[\mathrm{O}_{2}\right]\) ;

(d) decrease the volume of the container in which the reaction occurs;

(e) add a catalyst;

(f) increase temperature.

Text Transcription:

4 NH_3(g)+5 O_2(g) rightleftharpoons

4 NO(g)+6 H_2 O(g), Delta H=-904.4 kJ

[NH_3]

[H_2 O]

[O_2]