How are real gases different from ideal gases? real gases differ from ideal gases because in a real gas, a. the particles aren't always moving b. the particles don't bounce off walls c. the particles take up volume a. inter-molecular forces exist between particles b. the average energy depends only on the temperature c. the particles don't lose energy from collisions

Real gases are different from ideal gases because in a real gas:

C. The particles take up volume.

A. Inter-molecular forces exist between particles.

A real gas is also referred to as a non-ideal gas because inter-molecular forces of attraction exist between its particles.

This ultimately implies that, a real gas differ from an ideal gas because it does not behave or act as an ideal gas.

Basically, the characteristics of a real gas include the following:

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Real gases differ from ideal gases because, in a real gas,

C. The particles take up volume

A. Inter-molecular forces exist between particles

Explanation:

The particles of an ideal gas have no volume and no attractions for each other.

In a real gas, however, the molecules do have a measurable (but small) volume. For example, the volume of 1 mol an ideal gas at STP (0 °C and 1 bar) is 22.711 L. The molar volume of a real gas would be slightly greater than 22.711 L.

The molecules of real cases have intermolecular attractions for each other. On average, they will be slightly closer to each other, so the molar volume of a real gas will be slightly less than 22.711 L.

However, real gases are like ideal gases because their molecules

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)