Which statement is always true for a spontaneous reaction?

The process' spontaneity seems to be related to the transition from a highly organised system to a uniform, less ordered condition. Because of the exothermic nature of the reaction, the surroundings' entropy grows enough to more than make up for the system's negative entropy. As a result, the overall $\mathrm{\Delta }S=\mathrm{\Delta }{S}_{\text{surrounding }}-\mathrm{\Delta }{S}_{\text{system }}$entropy change is still positive.