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Question

5.1 g NH4SH is introduced in 3.0 L evacuated flask at 327oC. 30% of the solidNH4SH decomposed to NH3 and H2S as gases. The KP of the reaction at 327oC is
(R=0.082 L atm mol1,
molar mass of S=32 g mol1,
molar mass N=14 g mol1.


A

1×104atm2

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B

4.9×104atm2

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C

0.242atm2

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D
0.242×104atm2
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Solution

The correct option is C

0.242atm2


Correction option is C)

Moles of NH4SH=5.151=0.1 mol
NH4SH(s)NH3(g)+H2S(g)

Initially 0.1 0 0

At equil 0.1(1α)0.1α 0.1α

α=30%=0.3

So, number of moles equilibrium due to gaseous product

=0.1×0.3+0.1×0.3
=0.03+0.03

Now use PV = nRT
At equlibrium,

Ptotal×3lit=(0.03+0.03)×.082×600

Ptotal=0.984 atm

At equilibrium,

PNH3=PH2S=Ptotal2=0.492

Kp=PNH3×PH2S=0.492×0.492

Kp=0.242 atm2


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