Montgomery Wright
09/05/2024 · Junior High School
\( \quad \) Use the References to access important values if needed for this question. A student ran the following reaction in the laboratory at 705 K : \[ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) \] When she introduced 0.0389 moles of \( \mathrm{N}_{2}(g) \) and 0.0706 moles of \( \mathrm{H}_{2}(g) \) into a 1.00 liter container, she found the equilibrium concentration of \( \mathrm{H}_{2}(g) \) to be 0.0680 M . Calculate the equilibrium constant, \( K_{\mathrm{c}} \), she obtained for this reaction. \( K_{\mathrm{c}}= \)
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The equilibrium constant \( K_c \) is approximately 250.5.
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