Compute the value of - S at 298K for the reaction- H 2 g- 1 2 O 2 g- H 2 OgGiven that- - G-228-6kJ- H-241-8kJ

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Compute the v...

Question

Compute the value of $Δ S$ at $298 K$ for the reaction,
$H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (g)$
Given that, $Δ G = - 228.6 k J; Δ H = - 241.8 k J$

44.3 J K^{- 1}

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- 44.3 J K^{- 1}

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34.3 J K^{- 1}

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- 34.3 J K^{- 1}

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Similar questions

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

P C l_{5} (g) + H_{2} O (g) ⟶ P O C l_{3} (g) + 2 H C l (g)

P_{w h i t e} + (3 / 2) C l_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ P O C l_{3}; Δ H = - 135.5 k c a l

H_{2} (g) + C l_{2} (g) ⟶ + 2 H C l (g); Δ H = - 44.1 k c a l

P (w) + (5 / 2) C l_{2} (g) ⟶ P C l_{5} (g); Δ H = - 89.6 k c a l

H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ H_{2} O (g); Δ H = - 57.8 k c a l

H_{2}

H_{2} (g) + 1 / 2 O_{2} (g) = H_{2} O (g); Δ H = - 241.8 k J

C O (g) + 1 / 2 O_{2} (g) = C O_{2} (g); Δ H = - 283 k J

2 C u O (s) ⟶ {C u}_{2} O (s) + \frac{1}{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

112

H_{2} (g)

C O (g)

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

Δ H = - 241.8 k J

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

Δ H = - 283 k J

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