$A$ golf ball of mass $m$ has a speed of $50 \ m \ s^{-1}$. If the speed can be measured within an accuracy of $2 \%$,the uncertainty in the position is

What is indicated by $\psi$ for atomic and molecular orbitals? How is the molecular orbital obtained by the Schrodinger wave equation?

$A$ ball weighing $10 \, g$ is moving with a velocity of $90 \, ms^{-1}$. If the uncertainty in its velocity is $5 \, \%$,then the uncertainty in its position is ....... $\times 10^{-33} \, m$. (Rounded off to the nearest integer) [Given : $h = 6.63 \times 10^{-34} \, Js$]

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:

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

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