Blake Valdez
04/30/2023 · High School
Use the References to access important values if needed for this question. The equilibrium constant, \( K_{\mathrm{c}} \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K . \[ \mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g) \] If an equilibrium mixture of the three compounds in a 5.30 L container at 298 K contains 3.41 mol of \( \mathrm{NH}_{4} \mathrm{HS}(s) \) and 0.470 mol of \( \mathrm{NH}_{3} \) , the number of moles of \( \mathrm{H}_{2} \mathrm{~S} \) present is
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The number of moles of \( \mathrm{H}_2\mathrm{S} \) at equilibrium is approximately 0.0108 mol.
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