Which of the following is/are stable and won't decompose into their elements at standard conditions at 25 degrees C? (298 degrees kelvin)
CuO(s) ∆H= −157.3 S= 42.63 ∆G= −129.7
N2H4(l) ∆H= 50.63 S= 121.21 ∆G= 149.34
C6H12(l) ∆H= −156.4 S= 26.7 ∆G= 204.4
PCl3(g) ∆H= −287.0 S= 311.78 ∆G= −267.8
additional info: H and G are in kj/mol
S is in J/mol
H = enthalpy
S = Entropy
G = Gibbs Free Energy
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Verified answer
Assuming that the Gibbs free energy changes you list in the question are the standard Gibbs free energy of formation of the compounds, then all the compounds that have negative free energy changes are stable with respect to decomposition into their constituent elements at STP. A negative free energy for a reaction indicates that the reaction is spontaneous. In the case of a standard free energy of formation, the relevant reaction is that of the elements in their standard state reacting to form the specified compound.