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Enthalpy of Solution

The Δ Hof f...

Question

The $Δ H_{f}^{o}$ for $C O_{2}$ (g), $C O$ (g) and $H_{2} O (l)$ are -393.5, -110.5 and -241.8 kJ.mol $^{- 1}$ respectively. The standard enthalpy change ( in kJ) for the reaction $C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} O (l)$ is:

A

524.1

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B

41.2

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C

-262.5

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D

-41.2

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Solution

The correct option is C 41.2
$Δ H = Δ_{f} H (C O) + Δ_{f} H (H_{2} O) - Δ_{f} H (H_{2})$ $- Δ_{f} H (C O_{2})$
$= - 110.5 - 241.8 - 0 + 393.5$
$= - 352.3 + 393.5$
$Δ H = 41.2 k J$

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Similar questions

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 (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}^{o}

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

H_{2} O_{(g)}

- 393.5, - 110.5

- 241.8

k J . m o l^{- 1}

, respectively. The

Δ H_{f}^{o}

k J . m o l^{- 1}

] for the reaction,

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

Δ H_{f}^{0}

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

H_{2} O (g)

- 393.5, - 110.5

- 241.8 k J 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

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