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Question

Ammonium hydrogen sulphide dissociates according to the equation NH4HS(s)NH3(g)+H2S(g). If the observed pressure of the mixture is 1.12 atm at 106oC, what is the equilibrium constant Kp of the reaction?

A
0.314 atm2
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B
2.000 atm2
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C
1.000 atm2
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D
0.480 atm2
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Solution

The correct option is A 0.314 atm2
NH4HS(s)NH3(g)+H2S(g)t=000t=teqx atmx atm
since solid has no role in pressure

so, total pressure , PT=2x=1.12
x=0.56
So
Kp=PNH3×PH2S
Kp=x×x=x2

putting values,
KP=0.314 atm2


Theory:

Writing Kp:

Example 1:
N2(g)+3H2(g)2NH3(g)
Kp=(PNH3)2eq(PN2)eq(PH2)3eq


Example 2:

12H2(g)+12I2HI(g)

Kp=(PHI)eq(PH2)12eq(PI2)12eq

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