Calculate the uncertainty in the position of an electron if the uncertainty in its velocity is `5.7 xx 10^(5) m//sec` (`h = 6.6 xx 10^(-34) kg m^(2) s^(-1)`, mass of the electron `= 9.1 xx 10^(-31) kg`)

Explanation

To calculate the uncertainty in the position of an electron given the uncertainty in its velocity, we will use the Heisenberg Uncertainty Principle. The principle states that the product of the uncertainty in position (Δx) and the uncertainty in momentum (Δp) is equal to or greater than a constant divided by 4π:

\[ \Delta x \cdot \Delta p \geq \frac{h}{4\pi} \]

Where:
- \( h \) is the Planck's constant (\( 6.6 \times 10^{-34} \, \text{kg m}^2 \text{s}^{-1} \))
...