Question about stability of Ozone

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    Ozone Stability
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The enthalpy of formation for ozone (O3) is positive, and the change in entropy during its formation is negative due to a decrease in the number of gaseous moles. This results in a positive Delta G for all temperatures, indicating that the formation of ozone is non-spontaneous. Despite this, ozone exists because the equilibrium constant expression shows that while the reaction can occur, the equilibrium favors the formation of oxygen (O2). The discussion raises questions about the concept of spontaneity, particularly why a reaction with a positive Delta G is still considered non-spontaneous and what spontaneity truly means in thermodynamic terms.
Kshitij Kabeer
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The enthalpy of formation of O3 is positive. Change in entropy for the formation of O3 is also negative( as the number of gaseous moles is decreasing). This means that Delta G is positive for all temperatures. So formation of ozone should be non spontaneous at all temperatures. Then how does it exist?
 
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Have you looked at the expression for the equilibrium constant?
 
You mean Delta G=-RTlnK? Yes. So you mean to say that the reaction still occurs but equilibrium favours formation of O2. OK I get your point, So now my question is why do we say the reaction is non spontaneous when Delta G is positive? What is the meaning of spontaneity?
 

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