In graphite, each carbon atom is linked to three other carbon atoms by covalent bonds.
In diamond each carbon atom is linked to four other carbon atoms by covalent bonds.
There are Van der Waals forces between the layers of graphite but these are relatively weak in comparison to a covalent bond. And hence they shouldn't be able to increase the melting point of graphite to a temp. higher than that of diamond.
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In graphite, each carbon atom is linked to three other carbon atoms by covalent bonds. In diamond each carbon atom is linked to four other carbon atoms by covalent bonds. There are Van der Waals forces between the layers of graphite but these are relatively weak in comparison to a covalent bond. And hence they shouldn't be able to increase the melting point of graphite to a temp. higher than that of diamond.