Which of the following must be true for a spontaneous exothermic process? A)only that $\Delta$S_sys 0 C)both $\Delta$S_sys

Question

Which of the following must be true for a spontaneous exothermic process? A)only that $\Delta$S_sys < 0 B)only that $\Delta$S_sys > 0 C)both $\Delta$S_sys < 0 and the magnitude of $\Delta$S_sys < the magnitude of $\Delta$S_surr D)both $\Delta$S_sys < 0 and the magnitude of $\Delta$S_sys > the magnitude of $\Delta$S_surr E)either $\Delta$S_sys > 0 or $\Delta$S_sys < 0 and the magnitude of $\Delta$S_sys < the magnitude of $\Delta$S_surr

Quizplus · Accepted Answer

The text in the choices seems to be corrupted or incorrectly formatted, making it difficult to interpret the specific scientific symbols or terms intended. However, based on the context of the question regarding a spontaneous exothermic process, the correct answer generally involves principles related to thermodynamics. For a spontaneous exothermic process, it is typically true that the change in the system's Gibbs free energy ($\Delta G$) is less than zero ($\Delta G < 0$) for the process to be spontaneous, and the process being exothermic implies that the change in enthalpy ($\Delta H$) is less than zero ($\Delta H < 0$). However, without clear text, it's challenging to directly match these principles to the given choices. The selection of "E" is based on a standard interpretation that for spontaneous processes, either the system's entropy increases, or the energy released to the surroundings is sufficient to drive the process, which aligns with general thermodynamic principles for spontaneous reactions.

Which of the Following Must Be True for a Spontaneous Δ\DeltaΔ

Which of the Following Must Be True for a Spontaneous $\Delta$