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Chapter 18: Problem 51

Under what conditions does a substance have a standard entropy of zero? Can a substance ever have a negative standard entropy?

Short Answer

Expert verified
A substance has a standard entropy of zero at absolute zero temperature (0 Kelvin). As for the possibility of a negative standard entropy, it is not possible because entropy measures the disorder within a system and cannot drop below the most ordered state, which is represented by zero.

Step by step solution

01

Zero Entropy Condition

Standard entropy of a substance is zero at absolute zero temperature (0 Kelvin). This is a consequence of the Third Law of Thermodynamics, which states that the entropy of a perfectly organized crystalline substance is zero at absolute zero temperature. This is because, at 0 Kelvin, a perfect crystal has only one possible microstate and its energy is well defined, so it is completely ordered.
02

Possibility of Negative Standard Entropy

A substance cannot have a negative standard entropy. The second law of thermodynamics states that in an isolated system, entropy can only increase over time. In addition, entropy measures the number of specific ways in which a system may be arranged, often taken to be a measure of 'disorder'. The most orderly situation can be represented with a 0 value (all particles in one state), so you cannot have 'less than the most orderly state', hence negative entropy doesn't make physical sense.

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Most popular questions from this chapter

Consider the following Bronstead acid-base reaction at \(25^{\circ} \mathrm{C}\) : $$ \mathrm{HF}(a q)+\mathrm{Cl}^{-}(a q) \rightleftharpoons \mathrm{HCl}(a q)+\mathrm{F}^{-}(a q) $$. (a) Predict whether \(K\) will be greater or smaller than unity, (b) Does \(\Delta S^{\circ}\) or \(\Delta H^{\circ}\) make a greater contribution to \(\Delta G^{\circ} ?\) (c) Is \(\Delta H^{\circ}\) likely to be positive or negative?

State the third law of thermodynamics and explain its usefulness in calculating entropy values.

As an approximation, we can assume that proteins exist either in the native (or physiologically functioning) state and the denatured state $$\text { native } \rightleftharpoons \text { denatured }$$ The standard molar enthalpy and entropy of the denaturation of a certain protein are \(512 \mathrm{~kJ} / \mathrm{mol}\) and \(1.60 \mathrm{~kJ} / \mathrm{K} \cdot \mathrm{mol}\), respectively. Comment on the signs and magnitudes of these quantities, and calculate the temperature at which the process favors the denatured state.

Crystallization of sodium acetate from a supersaturated solution occurs spontaneously (see p. 426). What can you deduce about the signs of \(\Delta S\) and \(\Delta H ?\)

Comment on the statement: "Just talking about entropy increases its value in the universe."
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