Difference between diamond and graphite

What is the relation between diamond and graphite ?

Diamond and Graphite are

Explain the difference in properties of diamond and graphite on the basis of their structures.

Assertion : Among the carbon allotropes, diamond is an insulater, wherea, graphite is a good conductor of electricity. Reason : Hybridization of carbon in diamond and graphite are sp^3 and sp^2 , respectively.

Allotropes of carbon: There are three forms of carbon. i.e., diamond, graphite and fullerene which exxist in crystalline form. Graphite and diamond occur in nature. The structure of diamond is tetrahedral with sp^(3) hybridisation and diamond exist in 3-D netowrk solid. in graphite, carbon is sp^(2) hybridised. each carbon linked to other carbon linked to other carbon atom forms hexagonal ring. it has a layered structure. diamond and graphite are purest form of carbon. Fullerene constitute a new family of carbon allotropes. Consisting of large spheroidal molecule of compound with general formula C_(2n) . common fullerene C_(6),C_(70) , contain 5 and 6 membered rings. Q. Which of the following statement is incorrect for graphite?

At 5xx10^(5) bar pressure, density of diamond and graphite are 3 g//c c and 2g//c c respectively, at certain temperature T. (1 L. atm=100 J)

Diamond is

Compare the structure of diamond and graphite ?

The enthalpies of combustion of diamond and graphite are - 395.4 kJ and - 393.5 kJ respectively calculate the enthalpy of transformation from diamond to graphite.

Densities of diamond and graphite are 3.5 and 2.3 g mL^(-1) , respectively. The increase of pressure on the equilibrium C_("diamond") hArr C_("graphite")