What is the value of $\Delta v \cdot \Delta x$ for an electron? What does it indicate?

(N/A) According to Heisenberg's uncertainty principle,$\Delta x \cdot \Delta p \ge \frac{h}{4\pi m}$.
Substituting $\Delta p = m \cdot \Delta v$,we get $\Delta x \cdot \Delta v \ge \frac{h}{4\pi m}$.
For an electron,$m = 9.11 \times 10^{-31} \ kg$ and $h = 6.626 \times 10^{-34} \ J \cdot s$.
$\Delta x \cdot \Delta v \ge \frac{6.626 \times 10^{-34}}{4 \times 3.14 \times 9.11 \times 10^{-31}} \approx 5.79 \times 10^{-5} \ m^2 \ s^{-1}$.
This value indicates that for an electron,it is impossible to determine both the position and velocity simultaneously with absolute precision.