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Heat of Formation

The Δ f H 0 f...

Question

The $Δ_{f} H^{0}$ for $C O_{2} (g), C O (g) a n d H_{2} O (g)$ 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 reaction
$C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} O (g)$ is :

524.1

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+ 41.2

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-262.5

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- 41.2

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Solution

The correct option is B + 41.2
Given, $Δ_{f} H^{0} (C O_{2}) = - 393.5 k J m o l^{- 1}$
$Δ_{f} H^{0} (C O) = - 110.5 k J m o l^{- 1}$
$Δ_{f} H^{0} (H_{2}) = - 241.8 k J m o l^{- 1}$
$C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} (g)$
$Δ_{r} H$ is related to bond enthalpies of reactants and products in the gas phase reaction as
$Δ_{r} H = \sum Δ_{f} H^{0} (p r o d u c t s) - \sum Δ_{f} H^{0} (r e a c t a n t s) = Δ_{f} H^{0} (C O) + Δ_{f} H^{0} (H_{2}) - Δ_{f} H^{0} (C O_{2}) - Δ_{f} H^{0} (H_{2}) = - 110.5 - 241.8 - (- 393.5) = + 41.20 k J m o l^{- 1}$
hence the standard enthalpy change for the given reaction is $+ 41.20 k J m o l^{- 1}$

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Similar questions

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

Q. The

Δ H_{f}^{\circ}

for

C O_{2} (g)

C O (g)

and

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

is:

Q. The

Δ H_{t}^{\circ}

for

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

and

H_{2} O_{(g)}

are

- 393.5, - 110.5

and

- 241.8 k J m o l^{- 1}

respectively the standard enthalpy change (in

K J

) for the reaction

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

is:

Q. The

Δ_{f} H^{o}

for the

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

and

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)

Q. The

Δ H_{f}^{0}

for

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

and

H_{2} O (g)

are

- 393.5, - 110.5

and

- 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)

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Heat of Formation

Standard XII Chemistry

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The ΔfH0 for CO2 (g), CO(g) and H2O (g) are -393.5, -110.5 and -241.8 kJ mol−1 respectively. The standard enthalpy change (in kJ mol−1) for the reaction CO2 (g)+H2 (g)→CO (g)+H2O (g) is :

The $Δ_{f} H^{0}$ for $C O_{2} (g), C O (g) a n d H_{2} O (g)$ 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 reaction
$C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} O (g)$ is :