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Chapter 11: Problem 14

Explain how increasing the temperature of a gas increases its pressure.

Short Answer

Expert verified
Increasing temperature increases molecular speed, causing more frequent and forceful collisions with the container walls, thus raising gas pressure.

Step by step solution

01

Understanding the Kinetic Molecular Theory

The kinetic molecular theory states that gas consists of small particles in constant, random motion. The pressure of a gas results from collisions of gas molecules with the walls of their container.
02

Temperature and Molecular Speed

Temperature is a measure of the average kinetic energy of the gas molecules. As temperature increases, the average kinetic energy of the molecules increases, causing them to move faster.
03

Collision Frequency with Container Walls

With an increase in molecular speed due to higher temperature, the molecules collide more frequently and with more force against the walls of the container. This increases the rate and force of collisions.
04

Pressure Increase

Since pressure is defined as the force exerted per unit area by molecules impacting the container walls, the increased collision rate and force result in higher pressure inside the container.

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Key Concepts

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

Gas Pressure
The concept of gas pressure revolves around the interactions between gas molecules and the walls of their container. Gas pressure can be understood simply as the force exerted by these molecules when they hit the container walls.
  • A gas is made up of countless small particles that are always moving, as described by the kinetic molecular theory.
  • As these particles move around, they collide with the sides of the container, and each collision applies a force.
  • The accumulation of these impacts over the entire surface area of the container generates what we observe as gas pressure.
These continuous collisions mean that the pressure inside a container will vary based on how fast and how frequently these particles collide with the walls. It鈥檚 important to remember that the pressure will increase if the speed or frequency of the molecular collisions increases.
Temperature and Kinetic Energy
Temperature plays a crucial role in the movement of gas molecules. It isn鈥檛 just a measure of "hot" or "cold", but more scientifically, it reflects the average kinetic energy of the molecules within a substance.
  • In a gaseous state, when you increase the temperature, you are essentially pumping more energy into the molecules.
  • This additional energy boosts the speed at which the molecules move.
  • Imagine a room full of bouncing balls; if you give each ball more energy, they bounce around faster and cover more ground.
Thus, a direct relationship exists between temperature and the average kinetic energy: as the temperature rises, the molecules gain more energy and move at higher speeds. This is why in warmer conditions, gases can exert more pressure, as the molecules are more energetic and collide more forcefully with the container walls.
Molecular Collisions
Molecular collisions are a fundamental component of how gas pressure and temperature are related. The kinetic molecular theory highlights the constant, random motion of gas particles which cause these collisions.
  • Each collision is significant because it results in a transfer of momentum, contributing to the pressure exerted on the container walls.
  • As temperature increases, so does the frequency and force of these collisions because molecules are moving faster.
  • More energetic molecules due to higher temperatures lead to more frequent and robust collisions.
These collisions are essentially the "communication" that determines pressure. In summary, when the temperature rises, the increased kinetic energy of the molecules leads to more intense and frequent collisions, and hence, higher gas pressure. Understanding this mechanism helps explain why containers might feel more pressurized on warmer days.

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Most popular questions from this chapter

If \(10.0 \mathrm{~L}\) of neon gas exerts a pressure of 125 psi at \(373 \mathrm{~K}\), what is the number of moles of gas?

If oxygen gas in a steel container is at a pressure of \(5.00 \mathrm{~atm}\), what is the pressure expressed in each of the following units? (a) psi (b) \(\mathrm{cm} \mathrm{Hg}\)

A sealed container holds the gases \(\mathrm{H}_{2}, \mathrm{~N}_{2}\), and \(\mathrm{O}_{2}\). Which of these gases corresponds to each of the following descriptions? (a) highest kinetic energy (b) lowest kinetic energy (c) fastest molecules (d) slowest molecules

Calculate the final volume when \(5.00 \mathrm{~L}\) of argon gas undergoes a pressure change from 1.55 atm to 6.50 atm. Assume that the temperature remains constant.

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