An athlete whose mass is 70.0 kg drinks 16.0 ounces (454 g) of refrigerated water. The water is

step 1 Here in part A, water, temperature of water is equal to 35 degree Fahrenheit, that is 5 by 9 int

An athlete whose mass is 70.0 kg drinks 16.0 ounces (454 g)...

An athlete whose mass is 70.0 kg drinks 16.0 ounces $(454 \mathrm{g})$ of refrigerated water. The water is at a temperature of $35.0^{\circ} \mathrm{F}$. (a) Ignoring the temperature change of the body that results from the water intake (so that the body is regarded as a reservoir always at $98.6^{\circ} \mathrm{F}$ ), find the entropy increase of the entire system. (b) What If? Assume the entire body is cooled by the drink and the average specific heat of a person is equal to the specific heat of liquid water. Ignoring any other energy transfers by heat and any metabolic energy release, find the athlete's temperature after she drinks the cold water given an initial body temperature of $98.6^{\circ} \mathrm{F}$. (c) Under these assumptions, what is the entropy increase of the entire system? (d) State how this result compares with the one you obtained in part (a).

Key Concepts

Irreversible processes

Irreversible processes are those in which the system undergoes spontaneous changes that increase the total entropy, such as the mixing of fluids at different temperatures. Unlike reversible processes, these changes are not easily undone, and they lead to an overall increase in disorder according to the second law of thermodynamics.

Entropy

Entropy is a thermodynamic quantity that measures the degree of disorder or randomness in a system. It is affected by the transfer of heat and the irreversible nature of many real processes. In calculations, the change in entropy is typically determined by integrating the heat transfer divided by the temperature over the process, highlighting how energy is dispersed and energy quality diminished.

Specific heat capacity

Specific heat capacity is a property of a substance that indicates the amount of energy required to raise the temperature of a unit mass by one degree Celsius (or Fahrenheit). It is essential for determining how much energy is absorbed or released during temperature changes, which in turn affects the overall energy and entropy balance in thermal interactions.

Conservation of energy

The principle of conservation of energy states that energy cannot be created or destroyed but only transformed from one form to another. In thermal processes, this means that the heat lost by one part of the system must equal the heat gained by another when no external work is involved. This principle is used to determine the final temperature when two bodies of different temperatures are mixed.

Thermal equilibrium

Thermal equilibrium occurs when two or more systems in thermal contact exchange energy until they reach the same temperature, at which point there is no net heat flow between them. Reaching thermal equilibrium is a key consideration in problems involving the mixing of substances at different initial temperatures.

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