Each quantum mechanical wave function does not have a readily interpretable physical meaning,but the square of the wave function gives the . . . . . . of finding the electron at a certain point.

The uncertainty in the position of an electron $(\Delta x)$ is approximately $100 \ pm$. Calculate the uncertainty in momentum $(\Delta p)$ of the electron in $kg \ m \ s^{-1}$. $[h = 6.626 \times 10^{-34} \ J \ s]$

If the uncertainty in velocity is $\frac{1}{2m} \sqrt{\frac{h}{\pi}}$, then the ratio of uncertainty in position and momentum is (in $: 1$)

The uncertainties in the velocities of two particles,$A$ and $B$ are $0.05 \ ms^{-1}$ and $0.02 \ ms^{-1}$ respectively. The mass of $B$ is five times that of the mass of $A$. What is the ratio of uncertainties $\frac{\Delta x_A}{\Delta x_B}$ in their positions?

According to Heisenberg's uncertainty principle,the product of uncertainties in position and velocity for an electron of mass $9.1 \times 10^{-31} \ kg$ is

The uncertainty in position and velocity of a particle in motion are $1 \times 10^{-8} \ m$ and $6.627 \times 10^{-20} \ m/s$, respectively. The mass of the particle is $(h = 6.627 \times 10^{-34} \ J \cdot s)$