6th Edition 11.39

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Beatrice Petelo 1F
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6th Edition 11.39

Postby Beatrice Petelo 1F » Mon Jan 14, 2019 7:20 pm

The solutions manual says to add reactions 1 and 2 together. Where does the Cl2 go when you do this step?
Also, why do we multiply the two K values together?

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Re: 6th Edition 11.39

Postby marisaimbroane1J » Mon Jan 14, 2019 7:26 pm

Koverall of two reactions combined is equal to K1 times K2. I think this rule may be in the textbook, but my TA went over it in discussion. Cl2 is an intermediate in this case (product in one reaction and a reactant in the next), so it is not seen in the overall reaction.

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Re: 6th Edition 11.39

Postby Kate_Santoso_4F » Mon Jan 14, 2019 10:24 pm

Here is the rule based on the textbook:
If a chemical equation can be expressed as the sum of two or more chemical equations: The equilibrium constant for the overall reaction is the product of the equilibrium constants for the component reactions.
When you add the two reactions, Cl2 is present as a product in one equation and a reactant in another equation. Therefore, it cancels out to give you the overall reaction and you just multiple the two equilibrium constants for the two reactions together to find the K for the overall reaction.

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