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The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored...

The decomposition of crystalline N2O5 N2O5(s)⟶2NO2(g)+12O(g) is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ∘C we have the following values for the standard state enthalpy and free energy changes of the reaction: ΔH∘=+109.6kJ/mol ΔG∘=−30.5kJ/mol

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Expert Solution

we know G = H - T S

from above   G   =−30.5kJ/mol H = 109.6kJ/mol T = 25 + 273 K = 298 K   S = ?

−30.5kJ/mol =  109.6kJ/mol -  298 K   S

−30.5kJ/mol - 109.6kJ/mol =   -  298 K   S

140.1 kJ/mol = 298 K   S

S = 0.4701   kJ/mol k

in above raction as H =+ve it means that the value of    - T S must be greater than H so that

0 > H  - T S

and      G = - ve so that the reaction must be spontaneous or thermodynamically favored .

queen_honey_blossom answered 2 years ago
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