The product of uncertainty in the position and uncertainty in the velocity of a particle is $5.79 \times 10^{-5} \ m^2 \ s^{-1}$. If the uncertainty in the position is $1 \ nm$, what is the uncertainty in the measurement of its velocity in $m \ s^{-1}$?

  • A
    $5.79 \times 10^7$
  • B
    $5.79 \times 10^5$
  • C
    $5.79 \times 10^{-5}$
  • D
    $5.79 \times 10^4$

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Heisenberg's uncertainty principle is not applicable to which of the following?

In an atom,an electron is moving with a speed of $600 \, m/s$ with an accuracy of $0.005 \%$. The certainty with which the position of the electron can be located is $(h = 6.6 \times 10^{-34} \, kg \, m^2 s^{-1}, m_e = 9.1 \times 10^{-31} \, kg)$:

$A$ golf ball has a mass of $40 \, g$ and a speed of $45 \, m/s$. If the speed can be measured within an accuracy of $2 \%$,calculate the uncertainty in the position.

Assertion $(A)$: The probability of finding an electron in a small volume around a point $(x, y, z)$ at a distance $r$ from the nucleus is proportional to $\psi^2$.
Reason $(R)$: Subatomic particles possess both particle and wave nature.

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