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Grade 12Physical Chemistry

Ammonium hydrogen sulphide dissociates as follows NH4HS(s) NH3(g) + H2S(g) If solid NH4HS is placed in an evacuated flask at certain temperature it will dissociate until the total pressure is 600 torr. (a) Calculate the value of equilibrium constant for the dissociation reaction (b) Additional NH3 is introduced into the equilibrium mixture without changing the temperature until partial pressure of NH3 is 750 torr, what is the partial pressure of H2S under these conditions? What is the total pressure in the flask?

Profile image of Ashi
12 Years agoGrade 12
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2 Answers

Profile image of Naveen Kumar
11 Years ago
The reversible reaction is:
...............NH4HS(s) <,................>.NH3(g) + H2S(g)
….............a....................................0.............0............(initially)
...............a-p1.................................p1............p1.........(at equilibrium)
Given total pressure=600 torr
............p1+p1..=600
p1=300 torr
Kp=p(NH3)*p(H2S)=p1*p1=90000(torr)2
Now if the partial pressure of NH3=750 torr, let partial pressure of H2S=p2
Then, Kp=90000=750*p2
p2=Kp/750
and total pressure=p2+750 torr
Profile image of Nanda Kishoreu
8 Years ago
It is an reversible reaction so the formula. Is Kp =kc (true) to paver of Nso it come p2+750::::::::.........................................................................................................................

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