The dissociation of phosphorus pentachloride takes place at (250^{circ} mathrm{C}) as [ mathrm{PCl}_{5} ightleftharpoons mathrm{PCl}_{3}+mathrm{Cl}_{2} quad

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The dissociation of phosphorus pentachloride takes place at $250^{\circ} \mathrm{C}$ as

\[ \mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{3}+\mathrm{Cl}_{2} \quad K_{P}=1.8 \]

Calculate the pressure (in atm) that is necessary to obtain $50 \%$ conversion of $\mathrm{PCl}_{5}$.

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Introduction To Chemical Engineering Thermodynamics

ISBN: 9788120348974

2nd Edition

Authors: HALDER

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Question Posted: May 02, 2024 07:00 AM

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The dissociation of phosphorus pentachloride takes place at (250^{circ} mathrm{C}) as [ mathrm{PCl}_{5} ightleftharpoons mathrm{PCl}_{3}+mathrm{Cl}_{2} quad

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Basis 1 mathrmmol of mathrmPCl5 At equilibrium mathrmPCl...View the full answer

Introduction To Chemical Engineering Thermodynamics

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