Question

the graph above shows how a particular real gas deviates from ideal behavior at very high pressures. based on this information, which of the following is most likely the gas and gives the reason based on kinetic molecular theory? a h₂ because it has the smallest mass. b n₂ because its molecules have a triple bond. c ne because it has a completely filled valence shell. d so₂ because it has the largest molecular volume.

Explanation:

At high - pressures, real gases deviate from ideal behavior mainly due to the volume of the gas molecules themselves. According to kinetic - molecular theory, ideal gases assume that gas molecules have no volume. Real gases with larger molecular volumes deviate more from ideal behavior. Among the given options, $SO_2$ has the largest molecular volume compared to $H_2$, $N_2$, and $Ne$. The other reasons given for $H_2$, $N_2$, and $Ne$ (mass, bond type, and electron - shell configuration) are not the main factors causing the deviation from ideal behavior at high pressures.

Answer:

D. $SO_2$ because it has the largest molecular volume.