(C) The uncertainty in velocity is given by $\Delta v = \frac{0.005}{100} \times 600 = 0.03 \, m/s$. According to Heisenberg's uncertainty principle,$

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(C) The uncertainty in velocity is given by $\Delta v = \frac{0.005}{100} \times 600 = 0.03 \, m/s$. According to Heisenberg's uncertainty principle,$\Delta x \cdot \Delta v \geq \frac{h}{4\pi m}$. Substituting the values: $\Delta x = \frac{h}{4\pi m \Delta v} = \frac{6.626 \times 10^{-34}}{4 \times 3.1416 \times 9.11 \times 10^{-31} \times 0.03}$. $\Delta x = \frac{6.626 \times 10^{-34}}{3.432 \times 10^{-31}} \approx 1.93 \times 10^{-3} \, m$.

Class 11 Chemistry Structure of Atom Uncertainty principle and Schrodinger wave equation

Medium

An electron has a velocity of $600 \, m/s$ with an accuracy of $0.005 \%$. Calculate the uncertainty in the position of this electron.

A
$1.52 \times 10^{-4} \, m$
B
$5.10 \times 10^{-3} \, m$
C
$1.92 \times 10^{-3} \, m$
D
$3.84 \times 10^{-3} \, m$

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Structure of Atom

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Uncertainty principle and Schrodinger wave equation

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An electron has a velocity of $600 \, m/s$ with an accuracy of $0.005 \%$. Calculate the uncertainty in the position of this electron.

Similar Questions

Uncertainty in position of a $0.25 \ g$ particle is $10^{-5} \ m$. What is the uncertainty in its velocity? (Given: $h = 6.6 \times 10^{-34} \ J \ s$)

The simultaneous determination of the exact position and momentum of an electron is:

The uncertainty in the position and velocity of a particle are $10^{-10} \ m$ and $5.27 \times 10^{-24} \ ms^{-1}$ respectively. The mass of the particle is ............. $kg$. $(h = 6.625 \times 10^{-34} \ JS)$

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