Solid dissociates into and at a certain temperature, the equilibrium pressure is P atm. What will be the partial pressure (in atm) of when is pumped into the system so that its partial pressure become

Question

Solid $NH_4HS$ dissociates into $NH_3$ and $H_2S$ at a certain temperature, the equilibrium pressure is P atm. What will be the partial pressure (in atm) of $H_2S$ when $NH_3$ is pumped into the system so that its partial pressure becomes P atm?

Prashant Kotian · Accepted Answer

Correct answer: B. Reaction: \textbf{Step 1 — Initial equilibrium (no added gas):} At equilibrium total pressure = atm, with equal moles of NH and HS: $$ P_{\text{NH}_3} = P_{\text{H}_2\text{S}} = \frac{P}{2} $$ $$ K_p = P_{\text{NH}_3} \cdot P_{\text{H}_2\text{S}} = \frac{P}{2} \cdot \frac{P}{2} = \frac{P^2}{4} $$ \textbf{Step 2 — After adding NH until :} Let be the new equilibrium HS pressure. is unchanged. $$ K_p = P \cdot P_{\text{H}_2\text{S}}' = \frac{P^2}{4} $$ $$ P_{\text{H}_2\text{S}}' = \frac{P}{4} = 0.25P $$ \textbf{Answer: B} — Equilibrium pressure of HS is

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