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The average temperature in deserts is high during the day but quite cool at night, whereas that in regions along the coastline is more moderate. Explain.

Short Answer

Expert verified
Deserts have rapid heat absorption and loss, while coastal areas have moderated temperatures due to water's heat retention and higher humidity.

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01

Understand Heat Absorption

Deserts have sandy soils that do not retain heat well. During the day, they quickly absorb heat from the sun, causing temperatures to rise drastically. However, at night, the sand also loses heat rapidly, leading to cooler temperatures.
02

Analyze Heat Retention in Coastal Areas

Regions along the coastline have large bodies of water that absorb and retain heat more effectively than sand. Water heats up slowly during the day but also cools down slowly at night, maintaining a more even temperature.
03

Consider the Effects of Humidity

Coastal areas usually have higher humidity levels than deserts. The moisture in the air helps moderate temperature fluctuations by absorbing heat during the day and releasing it at night, preventing extreme temperature variations.

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Heat Absorption
When discussing temperature variations, particularly in different geographical regions, the concept of heat absorption is key. In desert environments, sandy soils are a prominent feature. Sand has a lower capacity to retain heat, meaning it absorbs solar heat rapidly during the day. This results in significant temperature increases, as heat from the sun is absorbed quickly. However, this rapid absorption comes with a flipside. Sand also loses heat just as quickly when the sun sets, leading to a steep drop in temperature at night. This quick release of heat is why deserts experience such notable temperature extremes between day and night.
For ease of understanding, consider how a metal pan heats up fast on a stove and then cools rapidly once removed from heat. Similarly, deserts have surfaces that heat and cool quickly due to their heat absorption properties. These properties are crucial in shaping desert climates, making sunlit days scorching hot and nights surprisingly cold.
Heat Retention
Heat retention explains the differences in temperature variation between coastlines and deserts. Coastal areas surround large bodies of water, which behave very differently from desert sands. Water has a high heat capacity, meaning it absorbs heat slowly and retains it for longer periods. This capacity leads to moderate temperatures, preventing the extremes seen in deserts. During the day, coastal waters absorb heat without significant temperature spikes. At night, water cools down much slower than sand, releasing retained heat gradually. This gradual release helps maintain a warm environment, even when the sun is not out.
Think of water like a big heat sponge. It absorbs heat calmly during the day and releases it gently at night. This property is beneficial for coastal areas, ensuring consistent temperatures that are comfortable throughout both day and night, unlike the sharp contrasts found in deserts.
Humidity Effects
Humidity plays a pivotal role in moderating temperature variations, especially in coastal regions. Humidity refers to the amount of moisture present in the air. Coastal areas generally have higher humidity levels compared to deserts. This moisture serves as a buffer against rapid temperature changes. During the day, humid air absorbs heat, which prevents temperatures from soaring too high. At night, the moisture in the air slowly releases stored heat, reducing the drop in temperature significantly.
In simple terms, think of humidity as a natural thermostat. When it's humid, the air holds onto heat more efficiently, releasing it when needed, much like an insulating blanket might. This natural ability to moderate temperature swings ensures that coastal climates are relatively stable, preventing the stark changes that occur in desert climates where humidity is notably absent.

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Most popular questions from this chapter

Ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) and gasoline (assumed to be all octane, \(\mathrm{C}_{8} \mathrm{H}_{18}\) ) are both used as automobile fuel. If gasoline is selling for \(\$ 2.20 / \mathrm{gal},\) what would the price of ethanol have to be in order to provide the same amount of heat per dollar? The density and \(\Delta H_{\mathrm{f}}^{\circ}\) of octane are \(0.7025 \mathrm{~g} / \mathrm{mL}\) and \(-249.9 \mathrm{~kJ} / \mathrm{mol}\), respectively, and of ethanol are \(0.7894 \mathrm{~g} / \mathrm{mL}\) and \(-277.0 \mathrm{~kJ} / \mathrm{mol}\) respectively \((1 \mathrm{gal}=3.785 \mathrm{~L})\).

A quantity of \(2.00 \times 10^{2} \mathrm{~mL}\) of \(0.862 \mathrm{M} \mathrm{HCl}\) is mixed with \(2.00 \times 10^{2} \mathrm{~mL}\) of \(0.431 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) in a constant-pressure calorimeter of negligible heat capacity. The initial temperature of the \(\mathrm{HCl}\) and \(\mathrm{Ba}(\mathrm{OH})_{2}\) solutions is the same at \(20.48^{\circ} \mathrm{C}\). For the process $$\mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)$$ the heat of neutralization is \(-56.2 \mathrm{~kJ} / \mathrm{mol}\). What is the final temperature of the mixed solution? Assume the specific heat of the solution is the same as that for pure water.

A quantity of \(85.0 \mathrm{~mL}\) of \(0.600 \mathrm{M} \mathrm{HCl}\) is mixed with \(85.0 \mathrm{~mL}\) of \(0.600 \mathrm{M} \mathrm{KOH}\) in a constant- pressure calorimeter. The initial temperature of both solutions is the same at \(17.35^{\circ} \mathrm{C}\), and the final temperature of the mixed solution is \(19.02^{\circ} \mathrm{C}\). What is the heat capacity of the calorimeter? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is \(-56.2 \mathrm{~kJ} / \mathrm{mol}\).

Consider the following data:$$\begin{array}{lcc}\text { Metal } & \text { Al } & \text { Cu } \\\\\hline \text { Mass }(\mathrm{g}) & 10 & 30 \\\\\text { Specific heat }\left(\mathrm{J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right) & 0.900 & 0.385 \\\\\text { Temnerature }{ }^{\circ}{ }^{\circ} \mathrm{C} \text { ) } & 40 & 60\end{array}$$ When these two metals are placed in contact, which of the following will take place? (a) Heat will flow from \(\mathrm{Al}\) to Cu because \(\mathrm{Al}\) has a larger specific heat. (b) Heat will flow from \(\mathrm{Cu}\) to \(\mathrm{Al}\) because \(\mathrm{Cu}\) has a larger mass. (c) Heat will flow from \(\mathrm{Cu}\) to \(\mathrm{Al}\) because \(\mathrm{Cu}\) has a larger heat capacity (d) Heat will flow from Cu to Al because Cu is at a higher temperature. (e) No heat will flow in either direction.

The work done to compress a gas is \(47 \mathrm{~J}\). As a result, \(93 \mathrm{~J}\) of heat is given off to the surroundings. Calculate the change in internal energy of the gas.

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