Calcium carbonate can exist in two distinctly different crystalline forms, called calcite and aragonite. The standard Gibbs free energy of formation for calcite at 298 K is ∆fG0 = -1128.79 kJ/mol, and the standard Gibbs free energy of formation for aragonite at 298 K is ∆fG0 = -1127.75 kJ/mol. Which crystalline form is the more thermodynamically stable at a temperature of 298 K and a pressure of 1 bar, and what would be the value of ∆rG0 for the calcite → aragonite transformation at 298 K?

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.