Graphite and diamond are both forms of carbon. Their standard molar entropies are: S graphite =

Graphite and diamond are both forms of carbon. Their standard molar entropies are:

ΔS^θgraphite = 5.70 J K^–1 mol^–1, ΔS^θ_diamond = 2.40 J K^–1mol^–1

a. i. Suggest why the standard molar entropy of graphite is greater than that of diamond.

ii. Calculate the entropy change of the process C_graphite → C_diamond at 298K

iii. Explain why you would be unlikely to make diamonds from graphite at atmospheric temperature and pressure.

b. The standard molar enthalpy change for C_graphite → C_diamond is +2.00 kJ mol^–1.

i. Calculate the total entropy change for this reaction at 25.0ºC.

ii. Explain why you would be unlikely to make diamonds from graphite at atmospheric temperature and pressure.

c. Graphite reacts with oxygen to form carbon dioxide. Would you expect the entropy of the products to be greater or less than the entropy of the reactants? Explain your answer.