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Question

For the reaction, X2O4(l)2XO2(g), ΔU=2.1 Kcal, ΔS=20 cal K1 at 300 K.
Hence, ΔG is:

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Solution

The change in Gibbs Free energy is given by
ΔH=ΔU+ΔngRT
where
ΔH is the enthalpy of the reaction
ΔS is the entropy of the reaction
and ΔU is the change in internal energy
Δng is the (number of gaseous moles in product) - (number of gaseous moles in reactant)=2-0=2
R is the gas constant =2 cal
But,
ΔH=(2.1×103)+(2×2×300)=3300calHence,ΔG=ΔH=TΔSΔG=3300(300×20)ΔG=2700cal=2.7cal

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