Consider the following reaction - Cgraphite - O2g - CO2g- H- -x1 cal Cdiamond-O2g- CO2g- H-x2calWhat is the heat of transition of graphite into diamond-

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Bond Order and Enthalpy

Consider the ...

Question

Consider the following reaction :
$C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g) : H = - x_{1} c a l$
$C (d i a m o n d) + O_{2} (g) \to C O_{2} (g) : H = - x_{2} c a l$
What is the heat of transition of graphite into diamond?

x_{1} + x_{2}

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x_{2} - x_{1}

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x_{1} - x_{2}

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x_{1} x_{2}

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Solution

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Δ H_{t}

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

Δ H = x k J

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

Δ H = y k J

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 O}_{2}

C_{g r a p h i t e} + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 399.5 k J

C_{d i a m o n d} + O_{2} (g) ⟶ C O_{2} (g); Δ H^{o} = - 395.4 k J

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 (d i a m o n d, s) + O_{2} (g) \to C O_{2} (g); △ H = - 94.3 k c a l

C (g r a p h i t e, s) + O_{2} (g) \to C O_{2} (g); △ H = - 97.6 k c a l

C (d i a m o n d, s) \to C (g r a p h i t e, s)

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