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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

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B

-676.4 kJ

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C

-110.4 kJ

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D

+110.4 kJ

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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

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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

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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

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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)

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Δ H = - 1058

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