(a) Can endothermic chemical reactions be spontaneous? (b) Can a process be spontaneous at one temperature and nonspontaneous at a different temperature? (c) Water can be decomposed to form hydrogen and oxygen, and the hydrogen and oxygen can be recombined to form water. Does this mean that the processes are thermodynamically reversible? (d) Does the amount of work that a system can doon its Id on the nath of the nrocese?

(a) Yes, endothermic chemical reactions can be spontaneous if the increase in entropy (\( ∆S \)) is large enough to overcome the positive enthalpy change (\( ∆H \)), resulting in a negative Gibbs free energy (\( ∆G \)). This is more likely to occur at higher temperatures due to the temperature-entropy term in the Gibbs free energy equation. (b) Yes, a process can be spontaneous at one temperature and nonspontaneous at a different temperature, as the Gibbs free energy (\( ∆G \)) is influenced by both enthalpy (\( ∆H \)) and entropy (\( ∆S \)) changes, as well as temperature (T). (c) The decomposition and recombination of water into hydrogen and oxygen are not thermodynamically reversible processes, as they have finite rates and energy losses and cannot fully reverse with no change to the system and its surroundings. (d) Yes, the amount of work that a system can do depends on the path of the process. Different process paths can lead to different conversion efficiencies and energy available for work, resulting in different amounts of work being done for the same initial and final states of a system.