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Introduction

Determine Δ...

Question

Determine $Δ H / k J$ for the following reaction using the listed enthalpies of reaction:
$4 C O (g) + 8 H_{2} (g) ⟶ 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l)$

Given that
$C (g r a p h i t e) + 1 / 2 O_{2} (g) ⟶ C O (g); Δ H / k J = - 110.5 k J$

$C O (g) + 1 / 2 O_{2} (g) ⟶ C O_{2} (g); Δ H / k J = - 282.9 k J$

$H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l); Δ H / k J = - 285.8 k J$

$C (g r a p h i t e) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H / k J = - 74.8 k J$

584.9 k J m o l^{- 1}

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279.8 k J m o l^{- 1}

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747.4 k J m o l^{- 1}

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925 k J m o l^{- 1}

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Solution

The correct option is C $747.4 k J m o l^{- 1}$
$4 C O (g) + 8 H_{2} (g) ⟶ 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l);$ $Δ H = ?$

$C (g r a p h i t e) + 1 / 2 O_{2} (g) ⟶ C O (g); Δ H_{1} = - 110.5 k J$

$C O (g) + 1 / 2 O_{2} (g) ⟶ C O_{2} (g); Δ H_{2} = - 282.9 k J$

$H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (I); Δ H_{3} = - 285.8 k J$

$C (g r a p h i t e) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H_{4} = - 74.8 k J$

Applying Hess's law,
$Δ H_{r} = - 3 \times Δ H_{1} + Δ H_{2} + 2 \times Δ H_{3} + 3 \times Δ H_{4}$

$Δ H_{r} = [3 (110.5) - 282.9 + 2 (- 285.8) + 3 (- 74.8)]$
$= - 747.4$

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Similar questions

Δ H / k J

4 C O (g) + 8 H_{2} (g) ⟶ 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l)

C (g r a p h i t e) + 1 / 2 O_{2} (g) ⟶ C O (g); Δ H / k J = - 110.5 k J

C O (g) + 1 / 2 O_{2} (g) ⟶ C O_{2} (g); Δ H / k J = - 282.9 k J

H_{2} (g) + 1 / 2 O_{2} (g) ⟶ H_{2} O (l); Δ H / k J = - 285.8 k J

C (g r a p h i t e) + 2 H_{2} (g) ⟶ C H_{4} (g); Δ H / k J = - 74.8 k J

Δ H / k J

2 C (s) + H_{2} (g) ⟶ C_{2} H_{2} (g)

2 C_{2} H_{2} (g) + 5 O_{2} (g) ⟶ 4 C O_{2} (g) + 2 H_{2} O (I) Δ H / k J = - 2600 k J

C (s) + O_{2} (g) ⟶ C O_{2} (g) Δ H / k J = - 390 k J

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (I) Δ H / k J = - 572 k J

Δ H / k J

2 N_{2} (g) + 5 O_{2} (g) ⟶ 2 N_{2} O_{5} (s)

N_{2} (g) + 3 O_{2} (g) + H_{2} (g) ⟶ 2 H N O_{3} (a q); Δ H / k J = - 414.0

N_{2} O_{5} (s) + H_{2} O (l) ⟶ 2 H N O_{3} (a q); Δ H / k J = - 86.0

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (l); Δ H / k J = - 571.6

C_{3} H_{8}

C_{3} H_{8} (g) + 5 O_{2} (g) ⟶ 3 C O_{2} (g) + 4 H_{2} O (g)

3 C (s) + 4 H_{2} (g) ⟶ C_{3} H_{8} (g) Δ H / k J = - 103.8

C (s) + O_{2} (g) ⟶ C O_{2} (g) Δ H / k J = - 393.5

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

Δ H / k J

2 N_{2} (g) + 5 O_{2} (g) ⟶ 2 N_{2} O_{5} (s)

N_{2} (g) + 3 O_{2} (g) + H_{2} (g) ⟶ 2 H N O_{3} (a q) Δ H / k J = - 414.0

N_{2} O_{5} (s) + H_{2} O (I) ⟶ 2 H N O_{3} (a q) Δ H / k J = - 86.0

2 H_{2} (g) + O_{2} (g) ⟶ 2 H_{2} O (I) Δ H / k J = - 571.6

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