What is the standard gibbs free energy for the transformation of diamond to graphite at 298 k? cdiamondâcgraphite?

Considering; graphite; standard enthalpy = 0 and entropy = 5.740; diamond standard enthalpy = 1.897 and entropy = 2.38.

Using the equation Delta G = Delta H - Temperature (DeltaS)

Delta H = enthalpy sum of products - enthalpy sum of reactants

Which will be; 0 - 1.897 = - 1.897 kJ/Mol

Delta S is the entropy sum; given by

5.740 - 2.38 = 3.36 J/Mol

We can convert Delta S from Joules to kilo Joules by dividing by 1000

we get; 0.00336 kJ/mol

We are given a temperature in kelvin which suits the calculations ((298 k)

Therefore; using the equation;

= - 1.897 - (298 * 0.00336) = - 2.90 kJ

Thus; the standard gibbs free energy will be; - 2.9 kJ