Which statement correctly reflects the relationship between spontaneity and work in thermodynamic processes?

The concept of spontaneity in thermodynamics is directly tied to the idea of whether a process can occur without the input of external energy. A spontaneous process is one that occurs naturally under a given set of conditions, resulting in an increase in the overall entropy of the system and its surroundings. In many cases, spontaneous processes are exothermic, releasing energy that can be converted into work.

Work in thermodynamics is defined as energy transferred when an object is moved by a force. While spontaneous processes can lead to the production of work, it’s essential to understand that not all spontaneous processes necessarily generate useful work. However, the correct statement emphasizes that spontaneous processes can indeed produce work, under appropriate conditions.

In contrast, non-spontaneous processes require energy input to occur, which can be provided in the form of work. Although non-spontaneous processes may become spontaneous when enough energy is supplied, this doesn't negate their initial classification as non-spontaneous.

Thus, the relationship indicated in the correct statement highlights the nature of spontaneous processes and their potential to produce work, aligning with the principles of energy transformation and thermodynamic spontaneity.