Physically, Why Is a Gas Molecule's Speed $v$ More Likely to Be Near

Physically, why is a gas molecule's speed $v$ more likely to be near $v_{p}$ than near zero?

A) There are fewer quantum states with smaller speeds than larger speeds.
B) The Boltzmann factor has a larger value near $\mathrm{v}=\mathrm{v}_{\mathrm{p}}$ than near $v=0$ .
C) We know that $\frac{1}{2} m\left[v^{2}\right]_{\text {avg }}=\frac{3}{2} k_{B} T$ , and $v_{p}$ is closer to $\left[v_{\text {avg }}^{2}\right]^{1 / 2}$ than zero is.