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Chapter 5: Problem 113

Use the kinetic theory of gases to explain why hot air rises.

Short Answer

Expert verified
Hot air rises because, according to the kinetic theory of gases, heating a gas causes its particles to move faster and collide more, leading to expansion. This expansion decreases the density of the air (mass per unit volume), making it lighter than surrounding colder, denser air. As a result, hot air rises when mixed with colder air due to differences in their densities.

Step by step solution

01

Understanding the Principles of Kinetic Theory

The kinetic theory of gases states that gases consist of numerous small particles, all of which are in continuous, random motion. The motion of these particles is directly related to the temperature of the gas – higher temperatures result in faster particle motion.
02

The Effect of Heat on a Gas

When a gas is heated, the additional energy leads to an increase in the speed of the gas particles. This increased speed means that the particles collide with each other and their container walls more frequently and with greater force. As a result, the gas expands – an effect called thermal expansion.
03

Why Hot Air Rises

The expansion of a hot gas leads to a decrease in its density (less mass per unit volume). In a mix with colder (and therefore denser) air, the hot, less dense air will rise above cold air due to the force of gravity acting differently on them. This effect, which can be observed in phenomena such as hot air balloons or convection currents, is why hot air rises.

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Most popular questions from this chapter

The volume of a gas is \(5.80 \mathrm{~L}\), measured at 1.00 atm. What is the pressure of the gas in \(\mathrm{mmHg}\) if the volume is changed to \(9.65 \mathrm{~L} ?\) (The temperature remains constant.)

Assuming that air contains 78 percent \(\mathrm{N}_{2}, 21\) percent \(\mathrm{O}_{2},\) and 1 percent \(\mathrm{Ar},\) all by volume, how many \(\mathrm{mol}-\) ecules of each type of gas are present in \(1.0 \mathrm{~L}\) of air at STP?

A sample of air contains only nitrogen and oxygen gases whose partial pressures are 0.80 atm and 0.20 atm, respectively. Calculate the total pressure and the mole fractions of the gases.

List the physical characteristics of gases.

A mixture of helium and neon gases is collected over water at \(28.0^{\circ} \mathrm{C}\) and \(745 \mathrm{mmHg}\). If the partial pressure of helium is \(368 \mathrm{mmHg}\), what is the partial pressure of neon? (Vapor pressure of water at \(28^{\circ} \mathrm{C}=\) \(28.3 \mathrm{mmHg} .)\)
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