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Gibbs Free Energy & Spontaneity

The H 0fCO2g,...

Question

$T h e △ H_{f}^{0}$
$C O_{2} (g), C O (g) a n d H_{2} O a r e - 393.5, - 110.5 a n d - 241.8 k J m o l^{- 1}$ respectively. The standard enthalpy change (in kJ) for the reaction $C O_{2} + H_{2} ⟶ C O + H_{2} O$ is.

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Solution

Given
$C + O_{2} ⟶ C O_{2}; △ H^{0} = - 393.5 k J . . . . . (i)$
$C + \frac{1}{2} O_{2} ⟶ C O; △ H^{0} = - 110.5 k J . . . . . (i i)$
$H_{2} + \frac{1}{2} O_{2} ⟶ H_{2} O; △ H^{0} = - 248.8 k J . . . . . (i i i)$
$(i i) + (i i i) - (i)$
$C O_{2} + H_{2} ⟶ C O + H_{2} O; △ H^{0} = 34.2$

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Similar questions

T h e △ H_{f}^{0}

C O_{2} (g), C O (g) a n d H_{2} O a r e - 393.5, - 110.5 a n d - 241.8 k J m o l^{- 1}

respectively. The standard enthalpy change (in kJ) for the reaction

C O_{2} + H_{2} ⟶ C O + H_{2} O

Δ H_{f}^{o}

C O_{2 (g)}

C O_{(g)}

H_{2} O_{(g)}

- 393.5

- 110.5

- 241.8

m o l^{- 1}

respectively the standard enthalpy change (in KJ) for the reaction

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

Δ H_{f}^{\circ}

C O_{2} (g)

C O (g)

H_{2} O (g)

are - 393.5, -110.5 and - 241.8 KJ

m o l^{- 1}

respectively.
The standard enthalpy change (in kJ) for the reaction

C O_{2} + H_{2} \to C O + H_{2} O

Δ_{f} H^{o}

C O_{2} (g), C O (g)

H_{2} O (l)

are -393.5, -110.5 and -241.8

k J m o l^{- 1}

respectively. The standard enthalpy change (in

k J m o l^{- 1}

) for the given reaction is :

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

Δ H_{f}^{o}

C O_{2}

C O

H_{2} O (l)

are -393.5, -110.5 and -241.8 kJ.mol

^{- 1}

respectively. The standard enthalpy change ( in kJ) for the reaction

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

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