**Core Concept**
An ideal gas is a hypothetical gas that obeys the ideal gas law (PV = nRT), where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. This concept is crucial in understanding the behavior of real gases.

**Why the Correct Answer is Right**
The ideal gas law is a mathematical model that describes the behavior of gases under different conditions. It assumes that gas molecules have no volume, there are no intermolecular forces, and the collisions between molecules are perfectly elastic. This means that the ideal gas law accurately predicts the behavior of gases at high temperatures and low pressures, where the molecules are far apart and there are minimal intermolecular forces.

**Why Each Wrong Option is Incorrect**
**Option A:** This option is incorrect because real gases do not behave ideally at high pressures and low temperatures, where the molecules are close together and intermolecular forces become significant.

**Option B:** This option is incorrect because the ideal gas law assumes that gas molecules have no volume, which is not true for real gases.

**Option C:** This option is incorrect because the ideal gas law does not take into account the intermolecular forces that exist between real gas molecules.

**Clinical Pearl / High-Yield Fact**
A useful mnemonic to remember the characteristics of an ideal gas is "PV = nRT": P - Pressure, V - Volume, n - Number of moles, R - Gas constant, T - Temperature.

**Correct Answer: C.**