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the equilibrium constants for the two reactions 2 HCl(g)    H2(g) + Cl2(g)             K1 = 4.36x10-2 and I2(g) + Cl2(g)    2 ICl(g)                 K2 = 8.92x10-6 are denoted K1 and K2 respectively, then the equilibrium constant, K3, for the reaction below is 2 HCl(g) + I2(g)    2 ICl(g) + H2(g)         K3= ?

the equilibrium constants for the two reactions 2 HCl(g)    H2(g) + Cl2(g)             K1 = 4.36x10-2 and I2(g) + Cl2(g)    2 ICl(g)                 K2 = 8.92x10-6 are denoted K1 and K2 respectively, then the equilibrium constant, K3, for the reaction below is 2 HCl(g) + I2(g)    2 ICl(g) + H2(g)         K3= ?

Chemistry
Chemistry
9th Edition
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Steven S. Zumdahl
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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If the equilibrium constants for the two reactions

2 HCl(g)    H2(g) + Cl2(g)             K1 = 4.36x10-2

and

I2(g) + Cl2(g)    2 ICl(g)                 K2 = 8.92x10-6

are denoted K1 and K2 respectively, then the equilibrium constant, K3, for the reaction below

is

2 HCl(g) + I2(g)    2 ICl(g) + H2(g)         K3= ?

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