Chapter 14: Problem 111
After the reaction \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftarrows 2 \mathrm{NH}_{3}(g)\) is run, an equilibrium mixture at \(300^{\circ} \mathrm{C}\) is \(0.25 \mathrm{M}\) in \(\mathrm{N}_{2}(g), 0.15 \mathrm{M}\) in \(\mathrm{H}_{2}(g)\), and \(0.090 \mathrm{M}\) in \(\mathrm{NH}_{3}(g)\). (a) What is the value of \(K_{\text {eq }}\) ? (b) Which way does the equilibrium shift when \(\mathrm{H}_{2}(g)\) is added? (c) What happens to the value of \(K_{\text {eq }}\) when \(\mathrm{H}_{2}(g)\) is added? (d) Suppose we write this reaction as: \(2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2}(g) \rightleftarrows 4 \mathrm{NH}_{3}(g)\) Now what is the value of \(K_{\text {eq }} ?\) (e) The equilibrium shifts to the right when the reaction mixture is cooled. Is this reaction exothermic or endothermic? Justify your choice.
Short Answer
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Key Concepts
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