For the change, $C_{d i a m o n d} ⟶ C_{g r a p h i t e}; Δ H = - 1.89 k J$ , if $6 g$ of diamond
and $6 g$ of graphite are separately burnt to yield $C O_{2}$ the heat liberated in first case is:

Less than in the second case by

1.89 k J

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Less than in the second case by

11.34 k J

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Less than in the second case by

14.34 k J

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More than in the second case by

0.945 k J

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Solution

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C_{d i a m o n d} ⟶ + C_{g r a p h i t e}; Δ H = - 1.89 k J

C O_{2}

C (g r a p h i t e) \to C (d i a m o n d), δ H = 1.9 k J .

C O_{2},

C (g r a p h i t e) \to C (d i a m o n d), △ H = 1.9 k J .

6

6

C O_{2}

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.

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For the change, Cdiamond⟶Cgraphite;ΔH=−1.89kJ, if 6g of diamond and 6g of graphite are separately burnt to yield CO2 the heat liberated in first case is: