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Heat of Formation

The heat of t...

Question

The heat of transition ( $Δ H_{t}$ ) of graphite into diamond would be,
where, $C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g)$ $Δ H = x k J$
$C (d i a m o n d) + O_{2} (g) \to C O_{2} (g)$ $Δ H = y k J$

x + y

kJ/mole

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x - y

kJ/mole

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y - x

kJ/mole

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None of these

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Solution

The correct option is B $x - y$ kJ/mole
To calculate:
$C (g r a p h i t e) \to C (d i a m o n d)$
Heat of reaction will be equal to the heat of transition
Given:
$C (g r a p h i t e) + O_{2} (g) \to C O_{2} (g)$ $Δ H = x k J$
$C O_{2} (g) \to C (d i a m o n d) + O_{2} (g)$ $Δ H = - y k J$
So, by adding the two, required $Δ H$ = $(x - y$ ) kJ/mole

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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.

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

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

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

$Δ H = - 94.05 k c a l m o l^{- 1}$

$C_{d i a m o n d} + O_{2} (g) \to C O_{2} (g); Δ H = - 94.50 k c a l m o l^{- 1}$ therefore

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

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