16. Around 10,000 tonnes of PCI5 is produced per year as it is used as an important chlorinating reagent.Given: 2P(g) + 3C12(g) 2PC13(g)K= 15.0PCI3(g) + Cl2(g)→ PCI5(g)K =4.0What is the value of the equilibrium constant for the reaction below?2P(g) + 5Cl½(g) → 2PCI5(g)a. 23b. 31С.240d. 60e.19

Answered: Image /qna-images/answer/e865ba94-4d57-4108-bb9a-71ea4bc7e61a.jpg

Given: 2P(g) + 3C12(g) →2PCI3(g) PCI5(g) K 15.0 PCI3(g) + Cl2(g) · K = 4.0 What is the value of the equilibrium constant for the reaction below? 2P(g) + 5Cl2(g) → 2PCI5(g) a. 23 b. 31 С. 240 d. 60 e. 19

Given: 2P(g) + 3C12(g) →2PCI3(g) PCI5(g) K 15.0 PCI3(g) + Cl2(g) · K = 4.0 What is the value of the equilibrium constant for the reaction below? 2P(g) + 5Cl2(g) → 2PCI5(g) a. 23 b. 31 С. 240 d. 60 e. 19

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 12.26PAE: The following data were collected for the reaction, H2(g) + L(g) ** - HI(g), at equilibrium at 25°C:...

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Question

16.

Around 10,000 tonnes of PCI5 is produced per year as it is used as an important chlorinating reagent.
Given: 2P(g) + 3C12(g) 2PC13(g)
K= 15.0
PCI3(g) + Cl2(g)→ PCI5(g)
K =4.0
What is the value of the equilibrium constant for the reaction below?
2P(g) + 5Cl½(g) → 2PCI5(g)
a. 23
b. 31
С.
240
d. 60
e.
19

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