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Postby MichelleTran3I » Wed Dec 06, 2017 9:33 pm

a) A sample of 2.0 mmol Cl2(g) was sealed into a 2.0-L reaction vessel and heated to 1000. K to study its dissociation
into Cl atoms. Use the information in Table 11.2 to calculate the equilibrium composition of the mixture. (b) If 2.0 mmol F2 was placed into the reaction vessel instead of the chlorine, what would be its equilibrium composition at 1000. K?
(c) Use your results from parts (a) and (b) to determine which is thermodynamically more stable relative to its atoms at 1000. K, Cl2 or F2.

How would you determine which one is more stable relative to its atoms? Thanks!

Jessica Yang 1J
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Joined: Fri Sep 29, 2017 7:03 am

Re: 11.45

Postby Jessica Yang 1J » Wed Dec 06, 2017 11:00 pm

Once you determine the K of both dissociations by using the ICE table, you figure out that the K of chlorine is smaller than the K of fluorine. As a result, you know that in dissociation equilibrium, chlorine favors its reactants more (since K = concentration of products/concentration of reactants) Since chlorine favors its reactants more, it is more stable in the Cl2 state (which is on the reactants side) than F2.

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