Pena Ortiz
03/27/2024 · Primary 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 . \[ \mathrm{NH}_{4} \mathrm{HS}(\mathrm{s}) \rightleftharpoons \mathrm{NH}_{3}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{~S}(\mathrm{~g}) \] Calculate the equilibrium concentration of \( \mathrm{H}_{2} \mathrm{~S} \) when 0.576 moles of \( \mathrm{NH}_{4} \mathrm{HS}(\mathrm{s}) \) are introduced into a 1.00 L vessel at 298 K . \( \left[\mathrm{H}_{2} \mathrm{~S}\right]= \) Submit Answer
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The equilibrium concentration of \( \mathrm{H}_2\mathrm{S} \) is 0.0134 M.
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