Consider the phase transformation process C(graphite) → C(diamond). The ∆G for this process at 1 bar pressure and a temperature of 298 K has a value of 2.900 kJ/mol, and the ∆S for the process under these same pressure and temperature conditions has a value of -3.36 J/K-mol. If you raised the temperature from 298 K to 1000 K, but kept the pressure constant at 1 bar, would this increase, decrease, or not change the thermodynamic stability of graphite versus diamond?

MCQs on thermodynamics in classical mechanics systems. Topics include the first, second, and third laws of thermodynamics, energy, work, enthalpy, and entropy, spontaneity, chemical potential, equilibrium, phase changes, and chemical kinetics.