Calculate - G o for the following reaction- COg- 1 2 O 2 g- CO 2 g- H o -282-84kJGiven- S CO 2 o -213-8J K -1 mol -1 - S COg o -197-9J K -1 mol -1 - S O 2 o -205-0J K -1 mol -1

Δ S ^ o =∑ S _ (products) ^ o ∑ S _ reactants ^ o =[ S _ CO _ 2 ^ o ] [ S _ CO(g) ^ o + 1 2 S _ O _ 2 ^ o ] =213 [197.9+ 1 2 × 205]= 86.6 ...

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Gibbs Free Energy & Spontaneity

Calculate Δ...

Question

Calculate $Δ G^{o}$ for the following reaction:
$C O (g) + \frac{1}{2} O_{2} (g) ⟶ {C O}_{2} (g); Δ H^{o} = - 282.84 k J$
Given, $S_{{C O}_{2}}^{o} = 213.8 J K^{- 1} {m o l}^{- 1}, S_{C O (g)}^{o} = 197.9 J K^{- 1} {m o l}^{- 1}, S_{O_{2}}^{o} = 205.0 J K^{- 1} {m o l}^{- 1}$

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△ G^{o}

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g); △ H^{o} = - 282.84 k J / m o l

S_{C O_{2}}^{o} = 213.8 J K^{- 1} m o l^{- 1}, S_{C O (g)}^{o} = 197.9 J K^{- 1} m o l^{- 1}, S_{O_{2}}^{o} = 205.0 J K^{- 1} m o l^{- 1}

Δ G^{o}

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

Δ H^{o} = - 282.84 k J

S_{C O_{2}}^{o} = 213.8

^{- 1}

^{- 1}

S^{o}_{C O (g)} = 197.9

^{- 1}

^{- 1}

S^{o}_{O_{2}} = 205.8

^{- 1}

^{- 1}

C H_{3} O H (l)

C H_{3} O H (l) + \frac{3}{2} O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (l)

Δ H^{o} = - 726

m o l^{- 1}

+ O_{2} (g) \to C O_{2} (g);

Δ_{c} H^{0} = - 393

m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l);

Δ_{t} H^{o} = - 286

m o l^{- 1}

25^{o} C

{F e}_{2} O_{3} (s) + 3 C_{g r a p h i t e} ⟶ 2 F e (s) + 3 C O (g); Δ H^{o} = 492 k J / m o l

F e O (s) + C_{g r a p h i t e} ⟶ F e (s) + C O (g); Δ H^{o} = 155.8 k J / m o l

C_{g r a p h i t e} + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 393.51 k J / m o l

C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 282.98 k J / m o l

F e O (s)

{F e}_{2} O_{3} (s)

Δ H

k J

C (g) + O_{2} (g) \to C O_{2} (g)

H_{2} O (g) + C (g) \to C O (g) + H_{2} (g)

Δ H = + 131 k J

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

Δ H = - 282 k J

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

Δ H = - 242 k J

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