Cgraphite-O2g- CO2g- - H-393-5kJ- - H of the reaction cannot be-

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Allotropes of Carbon

Cgraphite+O2g...

Question

$C_{g r a p h i t e} + O_{2 (g)} \to C O_{2 (g)}; Δ H = - 393.5 k J, Δ H$ of the reaction cannot be:

Heat of formation of

C O_{2}

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Heat of combustion of

C O_{2}

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Heat of reaction

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Heat of transition

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Solution

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Similar questions

Assertion- $C (g r a p h i t e) + O_{2 (g)} \to C O_{2 (g)}$ ,

$Δ H = - 393.5 k . J$

$C (d i a m o n d) + O_{2 (g)} \to C O_{2 (g)}$ ,

$Δ H = - 395.4 k . J$

Reason(R): graphite is more stable than diamond, so heat of combustion is less.

C_{(g r a p h i t e)} + \frac{1}{2} O_{2} \to C O; Δ H = - 110.5 k J

C O + \frac{1}{2} O_{2} \to {C O}_{2}; Δ H = - 283.2 k J

C_{(g r a p h i t e)} + O_{2} \to {C O}_{2}

C_{(g r a p h i t e)}

- 393.5 k J

{m o l}^{- 1}

{C O}_{2}

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

C_{(g r a p h i t e)} + O_{2 (g)} \to C O_{2 (g)}; Δ H = - 393.7 k J

C_{(d i a m o n d)} \to C_{(g r a p h i t e)}; Δ H = - 2.1 k J

C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g); Δ H = - 393.5 k J

H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (l); Δ H = - 286.2 k J

C_{2} H_{4} (g) + 3 O_{2} (g) \to 2 C O_{2} (g) + 2 H_{2} O (l); Δ H = - 1410.8 k J

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