What does the uncertainty principle state regarding the existence of a definite path or trajectory of an electron?

The Bohr model of the atom is contradicted by

Calculate the uncertainty in the position of a particle when the uncertainty in momentum is $1 \times 10^{-3} \, g \, cm \, sec^{-1}$.

Given below are two statements $:$
Statement $(I):$ It is impossible to specify simultaneously with arbitrary precision,both the linear momentum and the position of a particle.
Statement $(II) :$ If the uncertainty in the measurement of position and uncertainty in measurement of momentum are equal for an electron,then the uncertainty in the measurement of velocity is $\geq \sqrt{\frac{h}{4\pi}} \times \frac{1}{m}$ which simplifies to $\geq \frac{1}{2m} \sqrt{\frac{h}{\pi}}$. In the light of the above statements,choose the correct answer from the options given below $:$

In Heisenberg's uncertainty equation $\Delta x \times \Delta p \ge \frac{h}{4\pi}$,$\Delta p$ stands for:

When the uncertainty in the position of a moving particle is $0$,then the uncertainty in momentum $(p)$ is equal to: