Question:
The internal energy of an ideal gas is a function of which of the following ?
The internal energy of an ideal gas is a function of which of the following ?
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For a real gas, internal energy is a function of both temperature and volume (\( U = f(T, V) \)) due to intermolecular forces.
For an ideal gas, these forces are zero, simplifying the relationship to \( U = f(T) \).
For an ideal gas, these forces are zero, simplifying the relationship to \( U = f(T) \).
Updated On: Jul 21, 2026
- Pressure
- Volume
- Absolute Temperature
- Pressure, volume and temperature
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The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept:
The internal energy (\( U \)) of a substance represents the total kinetic and potential energy of its constituent molecules.
For an ideal gas, intermolecular forces of attraction are assumed to be non-existent.
As a result, there is no potential energy associated with molecular positions, and the internal energy consists solely of molecular translation, rotation, and vibration kinetic energy.
Step 2: Detailed Explanation:
According to Joule's law, the internal energy of a given mass of an ideal gas depends only on its temperature.
This can be mathematically expressed as:
\[ U = f(T) \]
Since temperature is a direct measure of the average kinetic energy of the gas molecules, any change in temperature leads directly to a change in internal energy.
Changes in pressure or volume at a constant temperature do not affect the internal energy of an ideal gas.
Therefore, the internal energy of an ideal gas is solely a function of its absolute temperature.
Step 3: Final Answer:
The internal energy of an ideal gas is a function of absolute temperature only.
The internal energy (\( U \)) of a substance represents the total kinetic and potential energy of its constituent molecules.
For an ideal gas, intermolecular forces of attraction are assumed to be non-existent.
As a result, there is no potential energy associated with molecular positions, and the internal energy consists solely of molecular translation, rotation, and vibration kinetic energy.
Step 2: Detailed Explanation:
According to Joule's law, the internal energy of a given mass of an ideal gas depends only on its temperature.
This can be mathematically expressed as:
\[ U = f(T) \]
Since temperature is a direct measure of the average kinetic energy of the gas molecules, any change in temperature leads directly to a change in internal energy.
Changes in pressure or volume at a constant temperature do not affect the internal energy of an ideal gas.
Therefore, the internal energy of an ideal gas is solely a function of its absolute temperature.
Step 3: Final Answer:
The internal energy of an ideal gas is a function of absolute temperature only.
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