For a certain reaction at 300 K , K = 10 , then ΔG ° for the same reaction is – ________ × 10 - 1 kJ mol - 1 . (Given R = 8 . 314 JK - 1 mol - 1 )

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The standard Gibbs free energy of the formation of a compound is basically the change of Gibbs free energy that is followed by the formation of one mole of that substance from its component element available at their standard states or the most stable form of the element which is at $25 °$ C and $100$ kPa. Its symbol is $Δ_{f} G ˚$ .

$ΔG ° = - RTℓnK$

$= - 8.314 \times 300 \ln (10)$

$= 5744.14 J / mole$

$= 57.44 \times 10^{- 1} kJ / mole$

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