P4(g) + 6 Cl2(g) →4 PCI3(g)If 0.680 moles of P4 is mixed with 2.99 moles of Cl2 in a 1.58-L rigid reaction vessel, what is the final pressure in the vessel after the reactiongoes to completion? The final temperature is 454. °C. Assume 100% yield.47.0 atm82.1 atm51.3 atm103. atmO 75.2 atm

Given that, P4(g) + 6Cl2(g) → 4PCl3(g) The initial number of moles of P4 = 0.680 moles The initial number of moles of Cl2 = 2.99 moles Volume of reaction vessel V = 1.58 L Final temperature T = 454oC = 727.15 K It is required to calculate the final pressure in the vessel after the reaction goes to completion.1 mol of P4 requires 6 mol of Cl2 for completion of the reaction 0.68 mol of P4 required 0.68 × 6 = 4.08 mol of Cl2 Only 2.99 mol of Cl2 is provided for the reaction. Hence Cl2 is the limiting reactant and P4 is the excess reactant. Number of moles of P4 reacted = 2.996 = 0.498 Number of moles of P4 unreacted = 0.68 - 0.498 = 0.182 mol Number of moles of PCl3 produced = 2.99 × 46 = 1.993 mol The total number of moles left after reaction: n = nP4 + nCl2 + nPCl3 n = 0.182 + 0 + 1.993 n = 2.175 molA rigid reaction vessel means the volume of the reaction vessel remains constant throughout the reaction. Assuming the gases as an ideal: PV = nRTP = nRTVP = 2.175 mol × 0.0821 atm.Lmol.K × 727.15 K1.58 LP = 82.1 atm Answer: final pressure in the vessel = 82.1 atm

Answered: P4(g) + 6 Cl2(g) →4 PCI3(g) If 0.680…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

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P4(g) + 6 Cl2(g) →4 PCI3(g)
If 0.680 moles of P4 is mixed with 2.99 moles of Cl2 in a 1.58-L rigid reaction vessel, what is the final pressure in the vessel after the reaction
goes to completion? The final temperature is 454. °C. Assume 100% yield.
47.0 atm
82.1 atm
51.3 atm
103. atm
O 75.2 atm

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