The uncertainty in the position of a particle of mass $0.25 \, kg$ is $10^{-5} \, m$. The uncertainty in its velocity is ...... $m/s$.

If the uncertainty in position and momentum are equal,then the uncertainty in velocity is .......

The uncertainty in the position of an electron moving with a velocity of $3 \times 10^4 \ cm/s$ is (given mass of electron $= 9.1 \times 10^{-28} \ g$,uncertainty in velocity $= 0.02 \ \%$).

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 $= 9.1 \times 10^{-31} \ kg, h = 6.63 \times 10^{-34} \ J \ s, \pi = 3.14]$

What is the uncertainty product $\Delta v \cdot \Delta x$ for a particle of mass $1 \ mg$? What does this imply?

What is the nature of the solution to the $Schrodinger$ wave equation for multi-electron atoms? How is it handled?