At 25 degree C in a closed system, ammonium hydrogen sulfide exists as the follo

Question

At 25 degree C in a closed system, ammonium hydrogen sulfide exists as the following equilibrium: NH_4 HS_(s) NH_3(g) + H_2 S_(g) (a) When a sample of pure NH_4HS_(s) is placed in an evacuated reaction and allowed to come to equilibrium at 25 degree C, total pressure is 0.257 atm. What is the value of K_p? (b) To this system, sufficient H_2S is injected until the pressure of H_2S is three times the value it had at equilibrium. What are the partial pressures of NH_3 and H_2S when equilibrium is re-established?

Explanation / Answer

( a ) NH4(g) NH3(g) + H2S(g)

initial moles 1 0 0

Equillibrium moles (1-x) x x

Total moles at equillibrium ( solid not included) = 2x

Mole freaction = x/2x = 1/2    1/2

Partial pressure = p/2     p/2

Kp =pNH3 x pH2S = p/2 X p/2 = P2/2

Given total pressure = 0.257

Therefore Kp = (0.257)2/2 = 0.066/2 = 0.033

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