Skip to main content
Ch.11 - Liquids and Intermolecular Forces
Chapter 11, Problem 83a

(a) When you exercise vigorously, you sweat. How does this help your body cool?

Verified Solution

Video duration:
1m
This video solution was recommended by our tutors as helpful for the problem above.
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Evaporation and Cooling

Evaporation is the process where liquid turns into vapor, which requires energy. When sweat evaporates from the skin's surface, it absorbs heat from the body, leading to a cooling effect. This is a crucial mechanism for thermoregulation, helping to maintain a stable internal body temperature during vigorous exercise.
Recommended video:
Guided course
04:50
Filtration and Evaporation

Thermoregulation

Thermoregulation is the process by which the body maintains its core internal temperature. During exercise, the body generates heat, and to prevent overheating, it activates mechanisms like sweating. This physiological response is vital for sustaining performance and preventing heat-related illnesses.

Role of Sweat Glands

Sweat glands are specialized structures in the skin that produce sweat, primarily composed of water and electrolytes. When the body temperature rises, these glands are stimulated to release sweat onto the skin's surface. The evaporation of this sweat is essential for effective cooling, as it helps dissipate excess heat generated during physical activity.
Recommended video:
Guided course
00:46
Writing Formulas
Related Practice
Textbook Question

The table below shows the normal boiling points of benzene and benzene derivatives.

(a) How many of these compounds exhibit dispersion interactions?

347
views
Textbook Question

The table below shows the normal boiling points of benzene and benzene derivatives. (e) Why is the boiling point of phenol the highest of all?

775
views
1
rank
Textbook Question

Use the normal boiling points propane (C3H8) -42.1 °C butane (C4H10) -0.5 °C pentane (C5H12) 36.1 °C hexane (C6H14) 68.7 °C heptane (C7H16) 98.4 °C to estimate the normal boiling point of octane (C8H18). Explain the trend in the boiling points.

2187
views
Textbook Question

(b) A flask of water is connected to a vacuum pump. A few moments after the pump is turned on, the water begins to boil. After a few minutes, the water begins to freeze. Explain why these processes occur.

634
views
Textbook Question

The following table gives the vapor pressure of hexafluorobenzene (C6F6) as a function of temperature: (a) By plotting these data in a suitable fashion, determine whether the Clausius–Clapeyron equation (Equation 11.1) is obeyed. If it is obeyed, use your plot to determine ∆Hvap for C6F6.

576
views
Textbook Question

Suppose the vapor pressure of a substance is measured at two different temperatures. (a) By using the Clausius–Clapeyron equation (Equation 11.1) derive the following relationship between the vapor pressures, P1 and P2, and the absolute temperatures at which they were measured, T1 and T2: (b) Gasoline is a mixture of hydrocarbons, a component of which is octane (CH3CH2CH2CH2CH2CH2CH2CH3). Octane has a vapor pressure of 13.95 torr at 25 °C and a vapor pressure of 144.78 torr at 75 °C. Use these data and the equation in part (a) to calculate the heat of vaporization of octane. (c) By using the equation in part (a) and the data given in part (b), calculate the normal boiling point of octane. Compare your answer to the one you obtained from Exercise 11.81. (d) Calculate the vapor pressure of octane at - 30 °C.

719
views