question_answer

\[5.1\text{ }g\text{ }N{{H}_{4}}SH\] is introduced in \[3.0L\] evacuated flask at \[327{}^\circ C.\,\]\[30%\] of the solid \[N{{H}_{4}}SH\] decomposed to \[N{{H}_{3}}\] and \[{{H}_{2}}S\] as gases. The \[{{K}_{p}}\] of the reaction at \[327{}^\circ C\] is (\[R=0.082L\,atm\text{ }mo{{l}^{-1}}{{K}^{-1}},\] Molar mass of \[S=32\text{ }g\text{ }mo{{l}^{-1}},\] molar mass of \[N=14\text{ }g\text{ }mo{{l}^{-1}}\])

A) \[0.242\times {{10}^{-4}}at{{m}^{2}}\]         

B) \[1\times {{10}^{-4}}at{{m}^{2}}\]

C) \[4.9\times {{10}^{-3}}at{{m}^{2}}\]    

D) \[0.242\text{ }at{{m}^{2}}\]

Correct Answer: A

Solution :

 \[{{K}_{P}}={{P}_{N{{H}_{3}}}}{{P}_{{{H}_{2}}S}}\]                   \[PV=nRT\]                                \[P\times 3=0.06\times 0.0821\times 600\] \[{{K}_{p}}=\frac{0.98}{2}\times \frac{0.98}{2}\]     \[P=\frac{0.06\times 0.0832\times 200}{3}\] \[{{K}_{p}}=0.243\]                 \[P=0.98\]