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Chapter 7: Problem 143

A clay pot containing water at \(25^{\circ} \mathrm{C}\) is placed in the shade on a day in which the temperature is \(30^{\circ} \mathrm{C} .\) The outside of the clay pot is kept moist. Will the temperature of the water inside the clay pot (a) increase; (b) decrease; (c) remain the same?

Short Answer

Expert verified
The temperature of the water inside the clay pot will decrease due to evaporation cooling.

Step by step solution

01

Understand Evaporation Cooling

Evaporation is a type of phase transition where a substance changes from a liquid state to a gas state. In this process, the particles of substance need to acquire enough energy to move from the liquid to the gas phase. As the water on the pot evaporates, the energy is taken from the pot, causing a decrease in the pot's (and subsequently the water inside) temperature.
02

Consider the Environmental Temperature

The current environmental temperature is \(30^{\circ} \mathrm{C}\) and the pot is kept in shade. This implies that there is minimal additional heat from the sun, therefore the primary heat source is the environmental air. The water inside the clay pot is initially at \(25^{\circ} \mathrm{C}\), which is less than the environmental temperature.
03

Evaluate Temperature Changes

Due to evaporation cooling, the pot's temperature will decrease further from the initial \(25^{\circ} \mathrm{C}\), and as the pot cools, it also cools the water inside. Therefore, it can be concluded that the temperature of the water inside the clay pot will decrease.

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Most popular questions from this chapter

Explain the important distinctions between each pair of terms: (a) system and surroundings; (b) heat and work; (c) specific heat and heat capacity; (d) endothermic and exothermic; (e) constant-volume process and constant-pressure process.

Can a chemical compound have a standard enthalpy of formation of zero? If so, how likely is this to occur? Explain.

A handbook lists two different values for the heat of combustion of hydrogen: \(33.88 \mathrm{kcal} / \mathrm{g} \mathrm{H}_{2}\) if \(\mathrm{H}_{2} \mathrm{O}(\mathrm{l})\) is formed, and \(28.67 \mathrm{kcal} / \mathrm{g} \mathrm{H}_{2}\) if \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) is formed. Explain why these two values are different, and indicate what property this difference represents. Devise a means of verifying your conclusions.

Refer to Example \(7-3 .\) Based on the heat of combustion of sucrose established in the example, what should be the temperature change \((\Delta T)\) produced by the combustion of \(1.227 \mathrm{g} \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) in a bomb calorimeter assembly with a heat capacity of \(3.87 \mathrm{kJ} /^{\circ} \mathrm{C} ?\)

James Joule published his definitive work related to the first law of thermodynamics in \(1850 .\) He stated that "the quantity of heat capable of increasing the temperature of one pound of water by \(1^{\circ} \mathrm{F}\) requires for its evolution the expenditure of a mechanical force represented by the fall of 772 lb through the space of one foot." Validate this statement by relating it to information given in this text.
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