Chapter 6, Problem 33TIS

Consider the decomposition of water $\left({\text{H}}_{\text{2}}\text{O}\right)$ to form hydrogen $\left({\text{H}}_{\text{2}}\right)$ and oxygen $\left({\text{O}}_{\text{2}}\right)$. At room temperature, the products of this reaction have less entropy than the reactants. Is this reaction thermodynamically favored? Justify your answer.