![]() ![]() For a perfect crystal at 0 K, the number of ways the total energy of a system can be. ![]() This is consistent with our molecular formula for entropy: S k lnW S k ln W. Since S = 0 corresponds to perfect order. The third Law of Thermodynamics states that the entropy of a pure substance in a perfect crystalline form is 0 J molK J m o l K at 0 K: S 0 K 0 S 0 K 0. The entropy of a pure crystalline substance at absolute zero (i.e. Nonetheless, the combination of these two ideals constitutes the basis for the third law of thermodynamics: the entropy of any perfectly ordered, crystalline substance at absolute zero is zero. In practice, absolute zero is an ideal temperature that is unobtainable, and a perfect single crystal is also an ideal that cannot be achieved. Such a state of perfect order (or, conversely, zero disorder) corresponds to zero entropy. The only system that meets this criterion is a perfect crystal at a temperature of absolute zero (0 K), in which each component atom, molecule, or ion is fixed in place within a crystal lattice and exhibits no motion (ignoring quantum effects). A perfectly ordered system with only a single microstate available to it would have an entropy of zero. The greater the molecular motion of a system, the greater the number of possible microstates and the higher the entropy. These forms of motion are ways in which the molecule can store energy. due to the reduction in the degrees of freedom, the system is more ordered after the reaction). There is a reduction in the disorder of the system (i.e.The reaction has resulted in a loss of freedom of the atoms (O atoms).Since they are now physically bonded to the other molecule (forming a new, larger, single molecule) the O atoms have less freedom to move around.The product of this reaction (\(NO_2\)) involves the formation of a new N-O bond and the O atoms, originally in a separate \(O_2\) molecule, are now connected to the \(NO\) molecule via a new \(N-O\) bond. ![]()
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