Moderators: Chem_Mod, Chem_Admin

Ryan Chang 1C
Posts: 105
Joined: Sat Aug 24, 2019 12:17 am


Postby Ryan Chang 1C » Wed Jan 08, 2020 4:59 pm

(a) 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 understand part a but can't seem to figure out part b and c. Could someone explain how to do these parts?

Vincent Leong 2B
Posts: 207
Joined: Fri Aug 09, 2019 12:15 am

Re: 5I.13

Postby Vincent Leong 2B » Wed Jan 08, 2020 6:39 pm

Cl2 is the more thermodynamically stable RELATIVE to its atoms because it has a lower K value. This indicates that there are more reactants or that more Cl2 exists than Cl and that means that less bonds of Cl2 are broken compared to F2. This indicates that relative to its atoms, Cl2 is more intact or tightly bond and therefore stable as a molecule.

Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 3 guests