Final answer:
The maximum work of a system cannot be obtained from real processes due to energy losses and inefficiencies inherent in irreversibility, as described by the second law of thermodynamics. Real processes have dissipative elements that further reduce efficiency and convert some work into heat rather than productive work output.
Step-by-step explanation:
The reason why the maximum work of a system can never be obtained from a real process is because real processes incur energy losses. This discrepancy between the theoretical maximum work and actual work done is due to several reasons. Primarily, according to the second law of thermodynamics, real processes are irreversible and therefore not perfectly efficient. Energy dissipation, often in the form of heat loss to the environment, occurs during such processes, inevitably resulting in less work output than theoretically possible.
Energy conservation is dictated by the first law of thermodynamics, ensuring that energy cannot be created or destroyed, only transformed. The second law of thermodynamics adds that, due to the inherent irreversibility of real processes and the efficiency limits of even the most ideal heat engines like the Carnot engine, not all heat can be converted into work.
Thus, when considering real-world applications, such as automobile engines or steam turbines, the presence of dissipative processes also play a significant role. These processes lead to further reductions in efficiency, as some work output is converted back into heat, rather than being used for productive work.