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Chapter 6: Problem 105

Why are cold, damp air and hot, humid air more uncomfortable than dry air at the same temperatures? (The specific heats of water vapor and air are approximately \(1.9 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\) and \(1.0 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\), respectively.

Short Answer

Expert verified
Cold, damp air and hot, humid air are more uncomfortable than dry air at the same temperatures because water vapor has a higher specific heat than air. It retains more heat in hot weather and more cold in cold weather, leading to prolonged discomfort. Additionally, human body cooling and warming mechanisms work less efficiently in damp and humid conditions.

Step by step solution

01

Comparing Specific Heats

Identify the specific heat capacities. Water vapor has a specific heat of \(1.9 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\) while air has \(1.0 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\). This means water can absorb and retain more heat than air.
02

Considering human body reactions

The human body responds differently to dry air and humid air because of the different specific heat capacities. In humid conditions, the large amount of water vapor in the air retains heat, making the air feel hotter. Furthermore, the human body cools down by evaporation of sweat, and this process is slower in humid conditions, leading to discomfort.
03

Factoring in weather conditions

Likewise, for cold weather, damp air feels cooler than dry air for the same reason. The water vapor in the air retains the cold more than in dry air. Additionally, the dampness in the air quickens the loss of heat from the body, causing discomfort.

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Most popular questions from this chapter

I he enthaipy of combustion benzo1c acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right)\) is commonly used as the standard for calibrating constant-volume bomb calorimeters; its value has been accurately determined to be \(-3226.7 \mathrm{~kJ} / \mathrm{mol}\). When \(1.9862 \mathrm{~g}\) of benzoic acid are burned in a calorimeter, the temperature rises from \(21.84^{\circ} \mathrm{C}\) to \(25.67^{\circ} \mathrm{C}\). What is the heat capacity of the bomb? (Assume that the quantity of water surrounding the bomb is exactly \(2000 \mathrm{~g} .)\)

Construct a table with the headings \(q, w, \Delta E,\) and \(\Delta H .\) For each of the following processes, deduce whether each of the quantities listed is positive \((+)\) negative \((-),\) or zero (0) . (a) Freezing of benzene. (b) Compression of an ideal gas at constant temperature. (c) Reaction of sodium with water. (d) Boiling liquid ammonia. (e) Heating a gas at constant volume. (f) Melting of ice.

The combustion of \(0.4196 \mathrm{~g}\) of a hydrocarbon releases \(17.55 \mathrm{~kJ}\) of heat. The masses of the products are \(\mathrm{CO}_{2}=1.419 \mathrm{~g}\) and \(\mathrm{H}_{2} \mathrm{O}=0.290 \mathrm{~g} .\) (a) What is the empirical formula of the compound? (b) If the approximate molar mass of the compound is \(76 \mathrm{~g}\), calculate its standard enthalpy of formation.

A piece of silver of mass \(362 \mathrm{~g}\) has a heat capacity of \(85.7 \mathrm{~J} /{ }^{\circ} \mathrm{C}\). What is the specific heat of silver?

The work done to compress a gas is \(74 \mathrm{~J}\). As a result, \(26 \mathrm{~J}\) of heat is given off to the surroundings. Calculate the change in energy of the gas.
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