Question bank/JEE Main/Chemistry

An amount of solid NH_4HS is placed in a flask already
containing ammonia gas at a certain temperature at 0.50 atm pressure.
Ammonium hydrogen sulphide decomposes to yield NH_3 and H_2S gases in
the flask. When the decomposition reaction reaches equilibrium, the
total pressure in the flask rises to 0.84 atm? The equilibrium constant
for NH_4HS decomposition at this temperature is:
Bksl NH_4HS dh,d ek=kk dks ¶ykLd ftl
rFkk 0.50 atm nkc ij vksj igq¡prh gS rks ¶ykLd esa dqy nkc 0.84 atm c<+ A blh
rki ij NH_4HS fo?kVu

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NH4HS(s) [IMAGE] NH3(g) + H2S(g)
Initial presens 0 0.5 0
At equi. 0 0.5+x x
Total pressure = 0.5 + 2x = 0.84 $\therefore\$ x = 0.17 atm
Kp = [IMAGE] = 0.11 atm

Source: Grass-G / CH-26 Chemistry Paper 1 15 Jan.docx