Real gases under typical conditions of pressure and temperature behave:
a) very nearly like an ideal gas
b) very unlike an ideal gas
c) completely unlike an ideal gas
d) exactly like an ideal gas

a) very nearly like an ideal gas

Explanation:

The reason real gases do not behave exactly like ideal gases is that certain properties that are associated with ideal gases do not always hold for real gases;

An example is that in ideal gases the collisions between the gas molecules are always elastic – meaning energy is conserved in the collisions. However, in real gases, some of the collisions are inelastic meaning some of the energy of the collision is tranformed into other forms of energy like heat energy.

Another assumption is that there are no forces of attraction or repulsion between molecules of ideal gases. However, in real gases there exists inter-molecular forces, though weak, between the molecules and are dependent on the distance between the molecules.

Again, while in ideal gases it is assumed that the molecules of the gas hold negligible volume compared to the volume of the gas, in reality, the volume of a  molecule of the gas is never absolutely zero; they do occupy some space.

idk what the question is about