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Heat of Formation

The heat of f...

Question

The heat of formation for a compound in the following reaction.
$H_{2} (g) + C l_{2} (g) \to 2 H C l (g) + 44 k c a l m o l^{- 1}$

- 44 k c a l m o l^{- 1}

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- 22 k c a l m o l^{- 1}

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11 k c a l m o l^{- 1}

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- 88 k c a l m o l^{- 1}

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Solution

The correct option is A $- 44 k c a l m o l^{- 1}$
$H_{2} (g) + C l_{2} (g) \to 2 H C l (g) + 44 k c a l m o l^{- 1}$
Heat of formation $= Δ H_{f} = - 44 k c a l m o l^{- 1}$

Suggest Corrections

Similar questions

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

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K_{c}

2 H C l (g) ⇌ H_{2} (g) + {C l}_{2} (g)

4 \times 10^{- 34}

25^{o} C

\frac{1}{2} H_{2} (g) + \frac{1}{2} {C l}_{2} (g) ⇌ H C l (g)

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

H_{2} (g) = 130.6, {C l}_{2} (g) = 233

H C l (g) = 186.7

298 K

1

H_{2} (g) + {C l}_{2} (g) \to 2 H C l (g)

H_{2} (g) + C l_{2} (g) \to 2 H C l (g)

Δ H

- 44

H_{2} (g) + C l_{2} (g) ⟶ 2 H C l (g)

298 K

S_{H_{2}}^{⊖} = 131 J K^{- 1} m o l^{- 1}

S_{C l_{2}}^{⊖} = 223 J K^{- 1} m o l^{- 1}

S_{H C l}^{⊖} = 187 J K^{- 1} m o l^{- 1}

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