What are the main reasons that gases deviate from ideal behavior?

[Select all that apply.]

Question

What are the main reasons that gases deviate from ideal behavior?

[Select all that apply.]

BlackTom AI · Accepted Answer

When evaluating why gases deviate from ideal behavior, we must consider the assumptions behind the ideal gas model and what real gases exhibit differently.
Option 1: 'Gas molecules have finite sizes.' Real gas molecules occupy a physical volume, so the available space for movement is reduced compared to an ideal gas assumption of point particles. This finite size leads to deviations especially at high pressures or low volumes where particle volume becomes non-negligible.
Option 2: 'Gas molecules do interact through intermolecular forces.' In real gases, attractions and repulsions between molecules (van der Waals forces, dipole interactions, etc.) influence energy, pressure, and compression behavior, causing deviations from ideal gas predictions, particularly at high pressures or low temperatures where such forces become more significant.
Option 3: 'Gas molecules do not interact through intermolecular forces.' This contradicts real-gas behavior; in reality, intermolecular forces do exist and contribute to deviations, so this statement is incorrect as a reason for deviation.
Option 4: 'The temperature is not proportional to the mean kinetic energy (ε) of the gas.' For an ideal gas, temperature is directly related to the mean kinetic energy. In deviations from ideality, the simple proportionality can break down due to interactions and finite size effects, but generally the foundational relationship T ∝ mean KE is still a guiding concept; the statement as a blanket claim is misleading because the proportionality remains a thermodynamic principle, whereas deviations arise from other factors. Therefore, this option is not a primary correct reason for deviation in the context of the ideal-gas model.
In summary, the correct considerations for deviations are the finite size of molecules and intermolecular forces, which align with options 1 and 2. The other statements do not accurately describe the main causes of deviation in real gases.

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