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Thermodynamic Stability

Posted: Mon Jan 13, 2020 5:06 pm
by Ryan Chang 1C
How do we determine if K, Cl2, of F2, is thermodynamically more stable in problem 5I.13?

Re: Thermodynamic Stability

Posted: Mon Jan 13, 2020 6:01 pm
by Daria MacAuslan 1H
Cl2 is more thermodynamically stable than F2 because of its smaller K vale, or equilibrium constant. This also means that it is going to dissociate less totally than F2 into singular atoms, which in turn makes it more stable (since it wants to stay in its original state of a diatomic molecule).

Re: Thermodynamic Stability

Posted: Mon Jan 13, 2020 6:27 pm
by AKatukota
It will be more thermodynamically stable if it has a smaller K.

Re: Thermodynamic Stability

Posted: Mon Jan 13, 2020 7:04 pm
by alicechien_4F
A molecule is more thermodynamically stable if it has a smaller K value. The smaller the K value, the less product there is relative to reactant. That means the reactant (in this case, Cl2 and F2) will dissociate less and remain as reactants.

Re: Thermodynamic Stability

Posted: Wed Jan 15, 2020 1:35 pm
by Caroline Zepecki
Smaller K value -> more thermodynamically stable

Re: Thermodynamic Stability

Posted: Thu Jan 16, 2020 3:07 pm
by 805307623
The more stable a system is, the lower the potential energy of it is. Chemical processes usually occur because they are thermodynamically favorable, meaning they go from high energy(less stable) to low energy(more stable).

Re: Thermodynamic Stability

Posted: Sat Jan 18, 2020 2:43 pm
by HuyHa_2H
You just look at the K value and compare them. Smaller K values indicate more thermodynamical stability and the opposite if the K value is bigger.