Here are the essential concepts you must grasp in order to answer the question correctly.
Ideal Gas Law
The Ideal Gas Law (PV=nRT) relates the pressure (P), volume (V), temperature (T), and number of moles (n) of a gas. It assumes that gas particles do not interact and occupy no volume, which is a good approximation under many conditions. Understanding this law is crucial for analyzing gas behavior, especially when considering how density changes with pressure.
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Density and Molar Mass Relationship
Density (d) is defined as mass per unit volume (d = m/V). For gases, density can also be expressed in terms of molar mass (M) and the Ideal Gas Law. The relationship shows that density is directly proportional to molar mass and inversely proportional to temperature and pressure, which is essential for understanding why d/P varies with pressure.
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Real Gas Behavior
Real gases deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces and the volume occupied by gas particles. This deviation can lead to non-constant relationships between density and pressure, as seen in the provided graph. Recognizing these deviations is important for interpreting experimental data and understanding gas properties under varying conditions.
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