CameraIcon

SearchIcon

MyQuestionIcon

119

You visited us 119 times! Enjoying our articles? Unlock Full Access!

Enthalpy of Combustion

What will be ...

Question

What will be the enthalpy of combustion of carbon to produce carbon monoxide on the basis of data given below?
$C_{(s)} + O_{2 (g)} \to C O_{2 (g)}$ $Δ H = - 393.4 k J$
$C O_{(g)} + \frac{1}{2} O_{2 (g)} \to C O_{2 (g)}$ $Δ H = - 283.0 k J$

A

+676.4 kJ

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

B

-676.4 kJ

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

C

-110.4 kJ

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

D

+110.4 kJ

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

Open in App

Solution

The correct option is A -110.4 kJ
$C + \frac{1}{2} O_{2} \to C O$ is obtained by (i) - (ii).
Therefore, $Δ H =$ -393.4 - (-283.0) = -110.4 kJ

Suggest Corrections

thumbs-up

0

Similar questions

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

C (g r a p h i t e) + \frac{1}{2} O_{2} (g) \to C O (g), Δ H = y k J m o l^{- 1}

C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g), Δ H = z k J m o l^{- 1}

Based on the given thermochemical equations, find out which one of the following algebric relationships is correct?

Δ H

k J

for the following reaction:

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

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

Δ H = + 131 k J

C O (g) + \frac{1}{2} O_{2} (g) \to {C O}_{2} (g)

Δ H = - 282 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (g)

Δ H = - 242 k J

Q. Given that: (i)

C (s) + O_{2} (g) \to C O_{2} (g); Δ H^{\circ} = - x k J

2 C O (g) + O_{2} (g) \to 2 C O_{2} (g); Δ H^{\circ} = - y k J

. The enthalpy of formation of carbon monoxide will be :

Q. Given the following thermos chemical reactions:

X O_{2} (s) + C O (g) \to X O (s) + C O_{2} (g)

Δ H = - 20.0

X_{3} O_{4} (s) + C O (g) \to 3 X O (s) + C O_{2} (g)

Δ H = + 6.0

3 X_{2} O_{3} (s) + C O (g) \to 2 X_{3} O_{4} (s) + C O_{2} (g)

Δ H = - 12.0

Δ H

in kJ for the reaction.

2 X O_{2} (s) + C O (g) \to X_{2} O_{3} (s) + C O_{2} (g)

.

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

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 1058

kJ/mole. Using the data, the heat of formation of ethanol is:

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Thermochemistry

CHEMISTRY

Watch in App

explore_more_icon

Explore more

Enthalpy of Combustion

Standard XII Chemistry

Join BYJU'S Learning Program

CrossIcon