A sample of solid NH$_4$HS is placed in a 1.0L closed vessel and allowed to equilibrate according to the following reaction: NH$_4$HS (s) = NH$_3$ (g) + H$_2$S (g) K$_c$ = 8.5 \times 10$^{-3}$ What is the equilibrium concentration (in M) of ammonia (NH$_3$)? 118 M 0.0085 M 0.082 M 0.092 M
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The equilibrium expression for the reaction NH3(s) = NH3(g) + H2S(g) is given by: K = [NH3(g)][H2S(g)] Show more…
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At 218 °C, Kc = 1.2 x 10^-4 for the equilibrium NH4SH(s) ⇌ NH3(g) + H2S(g). What is the equilibrium concentration of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218 °C and decomposes until equilibrium is reached? 0.15 M 0.020 M 0.015 M 0.011 M
Adi S.
At $218^{\circ} \mathrm{C}, K_{c}=1.2 \times 10^{-4}$ for the equilibrium $$ \mathrm{NH}_{4} \mathrm{HS}(s) \rightleftharpoons \mathrm{NH}_{3}(g)+\mathrm{H}_{2} \mathrm{~S}(g) $$ Calculate the equilibrium concentrations of $\mathrm{NH}_{3}$ and $\mathrm{H}_{2} \mathrm{~S}$ if a sample of solid $\mathrm{NH}_{4} \mathrm{HS}$ is placed in a closed vessel and decomposes until equilibrium is reached.
At 27°C, Kp = 0.095 for the equilibrium: NH4HS (s) ↔ NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains.
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