Final answer:
The correct criteria for spontaneity of a reaction is that the Gibbs free energy change (ΔG) must be negative (ΔG < 0). In the options given, B) ΔH > TΔS corresponds to a scenario where a process may be spontaneous, provided ΔG is negative as a result.
Step-by-step explanation:
The criteria of spontaneity for a chemical reaction may be written as ΔG < 0. This condition indicates that the Gibbs free energy change for a system must be negative for a process to occur spontaneously at constant temperature and pressure.
To predict spontaneity based on Gibbs free energy, one must consider the equation ΔG = ΔH - TΔS, where ΔH represents the change in enthalpy, T the absolute temperature in kelvins, and ΔS the change in entropy. Spontaneous processes usually have an increase in the entropy of the universe (ΔSuniv > 0), which means they are favored when the free energy of the system decreases.
Therefore, the answer to the question about the criteria of spontaneity is B) ΔH > TΔS, as it is implied that for a spontaneous reaction at constant temperature and pressure, ΔG must be negative. To reiterate, ΔG is derived from the enthalpy (ΔH) and the entropy (ΔS) changes, along with the absolute temperature (T), and a negative ΔG signifies a spontaneous process.