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Second Law of Thermodynamics

Following rea...

Question

Following reaction is spontaneous at $300 K$ .
$2 C u O (s) ⟶ C u_{2} O (s) + I / 2 O_{2} (g)$
$Δ H = - 144.6 k J m o l^{- 1}$ ; $Δ S = 0.116 k J m o l^{- 1}$ if true enter 1 else 0
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Solution

The correct option is A 1
A reaction is spontaneous if the value of the Gibbs free energy change is negative.
$2 C u O (s) ⟶ C u_{2} O (s) + I / 2 O_{2} (g)$
$Δ H = - 144.6 k J m o l^{- 1}$ ; $Δ S = 0.116 k J m o l^{- 1} K^{- 1}$
$Δ G = Δ H - T Δ S$ $= - 144.6 k J m o l^{- 1} - 300 \times 0.116 k J m o l^{- 1} K^{- 1}$ $= - 179.4 k J m o l^{- 1}$
Since the value of Gibbs free energy change $Δ G$ is negative' reaction is spontaneous.

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