The uncertainties in the velocities of particles $A$ and $B$ are $0.05 \, m/s$ and $0.02 \, m/s$,respectively. If the mass of particle $B$ is five times that of particle $A$,then the ratio of the uncertainties in their positions $\left( \frac{\Delta x_A}{\Delta x_B} \right)$ is equal to:

The uncertainty in the position of a moving bullet of mass $10 \ g$ is $10^{-5} \ m$. Calculate the uncertainty in its velocity.

If the position of the electron is measured within an accuracy of $\pm 0.002 \,nm$,calculate the uncertainty in the momentum of the electron. Suppose the momentum of the electron is $\frac{h}{4 \pi \times 0.05 \,nm}$,is there any problem in defining this value?

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

An accelerated electron has a speed of $5 \times 10^{6} \ m \ s^{-1}$ with an uncertainty of $0.02 \ \%$. The uncertainty in finding its location while in motion is $x \times 10^{-9} \ m$. The value of $x$ is $......$ (Nearest integer)
[Use mass of electron $= 9.1 \times 10^{-31} \ kg, h = 6.63 \times 10^{-34} \ J \ s, \pi = 3.14]$

The Bohr model of the atom is contradicted by