For the reaction COCl2g(?) ↔ ?o (?) + ?l2 2 (?), Kp was experimentally determined to be 0.0444 at 394.8 °C. assume that initially, n moles of COCl2(g) and no moles of CO(g) and Cl2(g) are present. a) Find the partial pressures of CO (g) and Cl2 (g) at equilibrium given 1.00 bar total pressure. b) What is the value of ∆rG at equilibrium? c) Determine ∆?G using the given equilibrium constant K.
For the reaction COCl2g(?) ↔ ?o (?) + ?l2 2 (?), Kp was experimentally determined to be 0.0444 at 394.8 °C. assume that initially, n moles of COCl2(g) and no moles of CO(g) and Cl2(g) are present. a) Find the partial pressures of CO (g) and Cl2 (g) at equilibrium given 1.00 bar total pressure. b) What is the value of ∆rG at equilibrium? c) Determine ∆?G using the given equilibrium constant K.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.18PAE: The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures...
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For the reaction COCl2g(?) ↔ ?o (?) + ?l2
2
(?), Kp was experimentally determined to be 0.0444 at 394.8 °C.
assume that initially, n moles of COCl2(g) and no moles of CO(g) and Cl2(g) are present.
a) Find the partial pressures of CO (g) and Cl2 (g) at equilibrium given 1.00 bar total pressure.
b) What is the value of ∆rG at equilibrium?
c) Determine ∆?G using the given equilibrium constant K.
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