For the common allotopes of carbon (grapnite and diamond) C(gr) C(dia) with equi

Question

For the common allotopes of carbon (grapnite and diamond) C(gr) C(dia) with equilibrium constant K = 0.32 The molar volumes 0f graphite and diamond are, respectively, 5.30 cm3/mol and 3.42 cm3/mol; deltaHr of diamond is 1.90kJ/mol. These dala suggest that the formation of diamond is favored at low temperatures and low pressures high temperatures and low pressures. low temperatures and high pressures high temperatures and high pressures. The equilibrium constant KC for the reaction A(g) + B(g) O(g) is 0.76 ay 150 degree C If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150 degree C, what will be the equilibrium concentration of C?

Explanation / Answer

C(graphite) <---------> C(diamond) ; delta H0f C(diamond) = 1.90 kJ/mole

Kc = [Cdiamond]/[Cgraphite] = 0.32

Also, molar volume of Cdiamond = 3.42 cm3 & Cgraphite = 5.30 cm3

Now, from the above information it is clear that , heat is required for the converion of graphite to diamond.

Also, the molar volume of diamond is lesser than that of carbon.Since pressure is inversely proportional to volume .

Hence it can be clearly interpreted that at high temperatures and high pressure, graphite can be converted to diamond

Hence the correct option is :-(D)

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