While doing 500 J of work, an ideal gas expands...

Name: Problem 5, Chapter 12: College Physics
Uploaded: 2021-05-03T21:45:30-08:00
Duration: 3 min 6 s
Channel: Shahab Ullah
Description: While doing 500 J of work, an ideal gas expands adiabatically to 1.5 times its initial volume. (a) The temperature of the gas (1) increases, (2) remains the same, (3) decreases. Why? (b) What is the change in the internal energy of the gas?

While doing 500 J of work, an ideal gas expands adiabatically to 1.5 times its initial volume. (a) The temperature of the gas (1) increases, (2) remains the same, (3) decreases. Why? (b) What is the change in the internal energy of the gas?

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Key Concepts

Temperature Changes in Adiabatic Expansion

In an adiabatic expansion, as the gas does work on its surroundings, its internal energy decreases, leading to a decrease in temperature. This outcome is consistent regardless of factors like the amount of work done or the specific volume change, as long as the process remains adiabatic.

Internal Energy

For an ideal gas, internal energy is directly related to its temperature. During an adiabatic expansion, the gas performs work without any heat input, which results in a decrease in its internal energy, and consequently, a drop in temperature.

Adiabatic Process

An adiabatic process is one in which no heat is exchanged with the surroundings. This means that the energy changes in the system are solely due to work done by or on the system. In such processes, any work done by the gas leads directly to a change in its internal energy, affecting the temperature of the gas.

First Law of Thermodynamics

The First Law of Thermodynamics states that the change in a system's internal energy equals the heat added to the system minus the work done by the system. In an adiabatic process, since no heat is exchanged, the change in internal energy is exactly the negative of the work done by the system.

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