Cyclopropane, a gas used with oxygen as a general anesthetic, is composed of 85.7% C and 14.3% H by mass. (b) Judging from its molecular formula, would you expect cyclopropane to deviate more or less than Ar from ideal-gas behavior at moderately high pressures and room temperature? Explain.

Verified step by step guidance

1. To determine if cyclopropane would deviate more or less from ideal-gas behavior compared to argon (Ar), we need to consider the factors that cause deviations from ideal behavior. These include intermolecular forces and the size of the molecules.
2. Ideal gases are assumed to have no intermolecular forces and occupy no volume. Real gases deviate from this behavior due to the presence of intermolecular forces and the finite volume of the gas particles.
3. Cyclopropane (C₃H₆) is a larger and more complex molecule than argon, which is a noble gas with a single atom. Cyclopropane has stronger intermolecular forces (such as van der Waals forces) due to its molecular structure.
4. At moderately high pressures, the volume of the gas particles and the intermolecular forces become significant. Cyclopropane, with its larger size and stronger intermolecular forces, is likely to deviate more from ideal-gas behavior than argon.
5. In summary, due to its molecular complexity and the presence of intermolecular forces, cyclopropane is expected to deviate more from ideal-gas behavior than argon at moderately high pressures and room temperature.

Key Concepts

Ideal Gas Law

The Ideal Gas Law describes the behavior of ideal gases through the equation PV=nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Ideal gases are assumed to have no intermolecular forces and occupy no volume, which allows them to perfectly follow this law under all conditions. However, real gases deviate from this behavior under high pressure and low temperature due to interactions between molecules and their finite volume.

Molecular Structure and Polarity

Cyclopropane is a small, cyclic hydrocarbon with a molecular formula of C3H6. Its structure leads to unique properties, including angle strain due to the 60-degree bond angles in the three-membered ring. This strain can affect the molecule's interactions with other molecules, influencing its behavior under various conditions, such as pressure and temperature, and potentially leading to deviations from ideal gas behavior.

Real Gas Behavior

Real gases deviate from ideal gas behavior primarily due to intermolecular forces and the volume occupied by gas molecules. At moderately high pressures, the volume of the gas becomes significant compared to the container, and attractive forces between molecules can lead to condensation. Cyclopropane, being a small and relatively polar molecule, is likely to experience these effects more than a noble gas, which behaves more ideally under similar conditions.