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Heat of Formation

Which of the ...

Question

Which of the following equations corresponds to the definition of enthalpy of formation at $298 K$ ?

C (g r a p h i t e) + 2 H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ C H_{3} O H (l)

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2 C (g r a p h i t e) + 4 H_{2} (g) + O_{2} (g) ⟶ 2 C H_{3} O H (l)

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C (d i a m o n d) + 2 H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ C H_{3} O H (l)

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C (g r a p h i t e) + 2 H_{2} (g) + \frac{1}{2} O_{2} (l) ⟶ C H_{3} O H (g)

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Solution

The correct option is A $C (g r a p h i t e) + 2 H_{2} (g) + \frac{1}{2} O_{2} (g) ⟶ C H_{3} O H (l)$

Graphite is a standard state of Carbon and $C H_{3} O H$ in liquid state is also a standard state. Hence, option A is correct because all the reactants and products must be in standard state.

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Similar questions

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}

C H_{3} O H (1) + \frac{3}{2} O_{2} (g) \to C O_{2} (g) + 2 H_{2} O (I); Δ, H^{⊖} = - 726 k J m o l^{- 1}

C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g); Δ_{c} H^{⊖} = - 393 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (I); Δ_{f} H^{⊖} = - 286 k J m o l^{- 1}

{C H}_{3} O H (l)

C_{(g r a p h i t e)} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}

C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ_{r} H^{o} = + 890.3 k J m o l^{- 1}

Δ_{r} H^{o}

298 K

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

C_{(g r a p h i t e} + O_{2} (g) \to C O_{2} (g); Δ_{r} H^{o} = - 393.5 k J m o l^{- 1}

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ_{r} H^{o} = - 285.8 k J m o l^{- 1}

C O_{2} (g) + 2 H_{2} O (l) \to C H_{4} (g) + 2 O_{2} (g); Δ^{r} H 6 o = + 890.3 k J m o l^{- 1}

D e l t a_{r} H^{o}

298 K

C_{(g r a p h i t e)} + 2 H_{2} (g) \to C H_{4} (g)

Determine $Δ U^{\circ}$ at 300 K for the following reaction using the listed enthalpies of reaction.

$4 C O (g) + 8 H_{2} (g) \to 3 C H_{4} (g) + C O_{2} (g) + 2 H_{2} O (l)$

$C (g r a p h i t e) + \frac{1}{2} O_{2} (g) \to C O (g); Δ {H_{1}}^{\circ} = - 110.5 k J$

$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g); Δ {H_{2}}^{\circ} = - 282.9 k J$

$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H_{3}^{0} = - 285.8 k J$

$C (g r a p h i t e) + 2 H_{2} (g) \to C H_{4} (g); Δ H_{4}^{0} = - 74.8 k J$

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