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Gibbs Free Energy & Spontaneity

For the react...

Question

For the reaction
$2 N O (g) + O_{2} (g) ⟶ 2 N O_{2} (g)$
Calculate $Δ G$ at $700 K$ when enthalpy and entropy changes are $- 113 k J {m o l}^{- 1}$ and $- 145 J K^{- 1} {m o l}^{- 1}$ respectively.

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Solution

We know that, $Δ G = Δ H - T Δ S$
Given that, $Δ H = - 113 k J {m o l}^{- 1} = - 113000 J {m o l}^{- 1}$
$Δ S = - 145 J K^{- 1} {m o l}^{- 1}$
$T = 700 K$
Substituting these values in the above equation
$G = - 113000 - 700 \times (- 145) = - 11500 J {m o l}^{- 1} = - 11.5 k J {m o l}^{- 1}$

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