Homework Question 5I.13

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Wendy 1E
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Homework Question 5I.13

Postby Wendy 1E » Wed Jan 08, 2020 11:21 pm

In an experiment, 2.0 mmol Cl2(g) was sealed into a reaction vessel of volume 2.0 L and heated to 1000. K to study its dissociation into Cl atoms. Use the information in Table 5G.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.

I'm only confused on part c. How can you tell which one is more stable?

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Re: Homework Question 5I.13

Postby WesleyWu_1C » Thu Jan 09, 2020 1:37 am

The way I could tell Cl2 was more stable was the fact that the K for equation for Cl2 <-> 2Cl was smaller than the K for the F2. A smaller K, means that compared to the other reaction, the reactant (Cl2) is favored more. In addition, if you compare the equilibrium concentrations of Cl2 to F2, you see that there is more Cl2 left over, which means it is more stable.

Brooke Yasuda 2J
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Re: Homework Question 5I.13

Postby Brooke Yasuda 2J » Thu Jan 09, 2020 10:20 am

When a question asks about which is more stable, it's like looking at lewis structures and determining which has stronger bonds and is thus, less likely to react. In this case, because there is more leftover unreacted Cl2 than F2, this shows that Cl2 is less likely to react into Cl and is, therefore, more stable.

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