MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Heat of Reaction

The Δ f H 0 f...

Question

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

A

524.1

No worries! We‘ve got your back. Try BYJU‘S free classes today!

B

41.2

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

C

-262.5

No worries! We‘ve got your back. Try BYJU‘S free classes today!

D

-41.2

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B 41.2
First write the balanced chemical equation for the formation of carbon dioxide, carbon monoxide and water :

$C (s) + O_{2} (g) \to C O_{2} (g); Δ H^{o} = - 393.5 k J m o l^{- 1} . . . . (i)$
$C (s) + \frac{1}{2} O_{2} (g) \to C O (g); Δ H^{o} = - 110.5 k J m o l^{- 1} . . . . (i i)$
$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H^{o} = - 241.8 k J m o l^{- 1} . . . . (i i i)$

then obtain the required equation by (ii) + (iii) - (i)
$C O_{2} (g) + H_{2} (g) \to C O (g) + H_{2} O (l) Δ H^{o} = + 41.2 k J m o l^{- 1}$

hence, the standard enthalpy of the reaction is $+ 41.2 k J m o l^{- 1}$

Suggest Corrections

thumbs-up

1

Similar questions

Δ_{f} H^{0}

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)

Δ H_{t}^{\circ}

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

K J

) 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)

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^{\circ}

C O_{2} (g), C O (g) a n d 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 is:

C O_{2} (g) + H_{2} (g) ⟶ C O (g) + H_{2} O (g)

Δ_{f} H^{o}

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

H_{2} O (l)

- 393.5, - 110.5

- 241.8 {kJ mol}^{- 1}

respectively. The standard internal energy change (in

{kJ mol}^{- 1}

) for the given reaction at

298 K

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

R = 8.3 J/K/mol

)

View More

Join BYJU'S Learning Program

explore_more_icon

Explore more

Heat of Reaction

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon