Ideal Gas vs Real Gases

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Definition of Ideal Gas

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An ideal gas is a theoretical gas composed of many particles that are in constant random motion and do not interact with each other, following the ideal gas law (PV=nRT).

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Definition of Real Gas

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A real gas is a gas that does not behave as an ideal gas due to interactions between particles and the volume occupied by the gas particles.

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Difference 1: Particle Interaction

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Ideal gases have no intermolecular forces, while real gases exhibit intermolecular forces.

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Difference 2: Volume of Gas Particles

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In ideal gases, the volume of gas particles is negligible, whereas in real gases, the volume of particles is significant.

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Difference 3: Behavior at High Pressure

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Ideal gases follow the ideal gas law at all pressures, while real gases deviate from this behavior at high pressures.

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Difference 4: Behavior at Low Temperature

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Ideal gases do not condense into liquids, while real gases can condense at low temperatures.

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Difference 5: Compressibility

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Ideal gases are perfectly compressible, while real gases have limits to their compressibility due to particle interactions.

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Difference 6: Molecular Speed

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In ideal gases, molecular speed is uniform and depends only on temperature, while in real gases, molecular speed varies due to intermolecular forces.

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Difference 7: Diffusion Rates

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Ideal gases diffuse at a constant rate, while real gases diffuse more slowly due to interactions between particles.

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Difference 8: Effect of Temperature

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Ideal gases show no change in behavior with temperature changes, while real gases can exhibit significant changes in behavior with temperature variations.