The Ideal Gas Equation Predicts That a Plot of the Pressure

The ideal gas equation predicts that a plot of the pressure times the volume of a gas versus the pressure of this gas should be a horizontal straight line at a fixed temperature. When these quantities are graphed for CO₂, however, we find that PV dips far below the theoretical straight line at first. This can be explained as follows.

A) The force of attraction between the CO₂ molecules makes the product of the pressure times the volume of this gas smaller than predicted from the ideal gas equation.
B) The volume of the CO₂ molecules makes the product of the pressure times the volume of this gas smaller than predicted from the ideal gas equation.
C) The force of attraction between the CO₂ molecules makes the product of the pressure times the volume of this gas larger than predicted from the ideal gas equation.
D) The volume of the CO₂ molecules makes the product of the pressure times the volume of this gas larger than predicted from the ideal gas equation.
E) There is no way to explain the difference between a real gas and the predictions of the ideal gas equation.