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Gibbs Free Energy & Spontaneity

Show that the...

Question

Show that the reaction,
$C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)$
at $300 K$ is spontaneous and exothermic, when the standard entropy change is $- 0.094 k J {m o l}^{- 1} K^{- 1}$ . The standard Gibbs free energies of formation for ${C O}_{2}$ and $C O$ are $- 394.4$ and $- 137 k J {m o l}^{- 1}$ respectively.

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Solution

The given reaction is
$C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)$
$Δ G^{o} (f o r r e a c t i o n) = G_{C O_{2}}^{o} - G_{C O}^{o} - G_{O_{2}}^{o} = - 394.4 - (- 137.2) - 0 = - 257 k J {m o l}^{- 1}$
$Δ G^{o} = Δ H^{o} - T {Δ S}^{o}$
$- 257.2 = Δ H^{o} - 298 \times (- 0.094)$
$Δ H^{o} = - 285.2 k J$

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Similar questions

Q. Show that the reaction

C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)

300 K

is spontaneous and exothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1}

. The values of standard Gibbs free energy of formation of

C O_{2}

C O

- 394.4

- 137.2 k J m o l^{- 1}

, respectively.

Q. Predict whether the reaction

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g)

at 300 K is spontaneous & exothermic or non-spontaneous & endothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1} .

The standard Gibb's free energies of formation for

C O_{2}

C O

- 394.4 a n d - 137.2 k J m o l^{- 1}

Q. Predict whether the reaction

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g)

at 300 K is spontaneous & exothermic or non-spontaneous & endothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1} .

The standard Gibb's free energies of formation for

C O_{2}

C O

- 394.4 a n d - 137.2 k J m o l^{- 1}

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)

The value of standard change in enthalpy for the above reaction on the basis of the following data is:

T = 300 K, Δ S^{o} = - 0.094 k J m o l^{- 1} K^{- 1}, Δ G_{f}^{o} (C O_{2}) = - 394.4 k J m o l^{- 1}

Δ G_{f}^{0} (C O) = - 137 k J m o l^{- 1}

Q. Standard enthalpy and standard entropy change for the oxidation of

{N H}_{3}

298 K

- 382.64 k J {m o l}^{- 1}

- 145.6 k J {m o l}^{- 1}

respectively. Standard Gibbs energy change for the same reaction at

298 K

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