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11 moles of \( \mathrm{N}_{2} \) and 12 moles of \( \mathrm{H}_{2} \) mixture reacted in 20 litre vessel at \( 800 \mathrm{~K} \). After equilibrium was reached, 6 mole of \( \mathrm{H}_{2} \) was present. \( 3.58 \) litre of liquid water is injected in equilibrium mixture and resultant gaseous mixture suddenly cooled to \( 300 \mathrm{~K} \). What is the final pressure of gaseous mixture? Neglect vapour pressure of liquid solution. Assume (i) all \( \mathrm{NH}_{3} \) dissolved in water (ii) no change in volume of liquid (iii) At \( 300 \mathrm{~K} \) no reaction takes place between \( \mathrm{N}_{2} \) and \( \mathrm{H}_{2} \)
\begin{tabular}{|l|l|l|}
\hline \( \mathrm{N}_{2}: 11 \) mole & \( \mathrm{T}=800 \mathrm{~K} \) \\
\cline { 2 - 4 } \( \mathrm{H}_{2}: 12 \) mole & \( \mathrm{V}=20 \mathrm{~L} \) & \( \mathrm{~N}=300 \mathrm{~K}: \mathrm{P}=? \) \\
\hline
\end{tabular}
Initial condition
(a) \( 18.47 \mathrm{~atm} \)
(b) \( 60 \mathrm{~atm} \)
(c) \( 22.5 \mathrm{~atm} \)
(d) 45 atm
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