A student ran the following reaction in the laboratory at 479 K:PCI3(g) + Cl₂(g) =PC15(g)When she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial partial pressure of PCI3 was 2.13 atm and the initial partial pressure of Cl₂ was 1.34 atm, she foundthat the equilibrium partial pressure of PCI5 was 1.12 atm.Calculate the equilibrium constant, Kp, she obtained for this reaction.KpSubmit AnswerRetry Entire Group8 more group attempts remaining

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udent ran the following reaction in the laboratory at 479 K: (g) + Cl₂(9) ⇒PCI5(9) n she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial the equilibrium partial pressure of PCI5 was 1.12 atm. ulate the equilibrium constant, Kp, she obtained for this reaction. mit Answer Retry Entire Group 8 more group attempts remaining

udent ran the following reaction in the laboratory at 479 K: (g) + Cl₂(9) ⇒PCI5(9) n she introduced PCI3(g) and Cl₂(g) into a 1.00 L evacuated container, so that the initial the equilibrium partial pressure of PCI5 was 1.12 atm. ulate the equilibrium constant, Kp, she obtained for this reaction. mit Answer Retry Entire Group 8 more group attempts remaining

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 33P

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Similar questions

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