The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K.\[\text{NH}_4\text{HS(s)} \rightleftharpoons \text{NH}_3\text{(g)} + \text{H}_2\text{S(g)}\]Calculate the equilibrium concentration of \(\text{H}_2\text{S}\) when 0.532 moles of \(\text{NH}_4\text{HS(s)}\) are introduced into a 1.00 L vessel at 298 K.\[[\text{H}_2\text{S}] = \boxed{\phantom{00}} \text{M}\]

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The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH,HS(s) NH3(g) + H,S(g) Calculate the equilibrium concentration of H2S when 0.532 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] = M

The equilibrium constant, K, for the following reaction is 1.80×10-4 at 298 K. NH,HS(s) NH3(g) + H,S(g) Calculate the equilibrium concentration of H2S when 0.532 moles of NH,HS(s) are introduced into a 1.00 L vessel at 298 K. [H2S] = M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

The equilibrium constant, \( K_c \), for the following reaction is \( 1.80 \times 10^{-4} \) at 298 K.

\[
\text{NH}_4\text{HS(s)} \rightleftharpoons \text{NH}_3\text{(g)} + \text{H}_2\text{S(g)}
\]

Calculate the equilibrium concentration of \(\text{H}_2\text{S}\) when 0.532 moles of \(\text{NH}_4\text{HS(s)}\) are introduced into a 1.00 L vessel at 298 K.

\[[\text{H}_2\text{S}] = \boxed{\phantom{00}} \text{M}\]

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