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Given that $C_{(graphite)}$ ® C(g); DH = +716.7 KJ.C(diamond) ® C(g) ; DH = 714.8 KJ. The DH for the following reaction is $C_{(graphite)}$ ® $C_{(deamond)}$

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1.9 KJ

-1.9 KJ

Zero

714.8 KJ

answer is A.

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Detailed Solution

$C_{(graphite)}$ ® C(g); DH = +716.7 KJ

$C_{(deamond)}$ ® C(g) DH = 714.8 KJ

For $C_{(graphite)}$ ® $C_{(deamond)}$

DH = 716.7 - 714.8

DH = 1.9 kJ

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