(A) According to Heisenberg's Uncertainty Principle:$\Delta x \cdot \Delta p \geq \frac{h}{4 \pi m}$Given:$\Delta x = 0.001 \ nm = 10^{-12} \ m$$m = 9

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(A) According to Heisenberg's Uncertainty Principle:$\Delta x \cdot \Delta p \geq \frac{h}{4 \pi m}$Given:$\Delta x = 0.001 \ nm = 10^{-12} \ m$$m = 9.11 \times 10^{-31} \ kg$$h = 6.626 \times 10^{-34} \ J \cdot s$Substituting the values:$\Delta v \geq \frac{6.626 \times 10^{-34}}{4 \times 3.1416 \times 9.11 \times 10^{-31} \times 10^{-12}}$$\Delta v \geq \frac{6.626 \times 10^{-34}}{1.144 \times 10^{-41}}$$\Delta v \geq 5.79 \times 10^7 \ m/s$

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

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$A$ microscope using appropriate photons is engaged to track an electron in an atom within a distance of $0.001 \ nm$. What will be the uncertainty involved in measuring its velocity?

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A
$5.79 \times 10^7 \ m/s$
B
$5.79 \times 10^6 \ m/s$
C
$4.79 \times 10^7 \ m/s$
D
$3.7 \times 10^6 \ m/s$

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Structure of Atom

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Uncertainty principle and Schrodinger wave equation

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If the uncertainty in the position of an electron is associated with an uncertainty in momentum of $2 \times 10^{-17} \ g \ cm \ s^{-1}$,what will be the uncertainty in the velocity of the electron?

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The uncertainty in momentum of an electron is $1 \times 10^{-5} \ kg \ m/s$. The uncertainty in its position will be $(h = 6.63 \times 10^{-34} \ Js)$.

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The measurement of the electron position is associated with an uncertainty in momentum,which is equal to $1 \times 10^{-18} \ g \ cm \ s^{-1}$. The uncertainty in electron velocity is (mass of an electron is $9 \times 10^{-28} \ g$):

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When the uncertainty in the position of a moving particle is $0$,then the uncertainty in momentum $(p)$ is equal to:

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

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$A$ microscope using appropriate photons is engaged to track an electron in an atom within a distance of $0.001 \ nm$. What will be the uncertainty involved in measuring its velocity?

Similar Questions

If the uncertainty in the position of an electron is associated with an uncertainty in momentum of $2 \times 10^{-17} \ g \ cm \ s^{-1}$,what will be the uncertainty in the velocity of the electron?

The uncertainty in momentum of an electron is $1 \times 10^{-5} \ kg \ m/s$. The uncertainty in its position will be $(h = 6.63 \times 10^{-34} \ Js)$.

The measurement of the electron position is associated with an uncertainty in momentum,which is equal to $1 \times 10^{-18} \ g \ cm \ s^{-1}$. The uncertainty in electron velocity is (mass of an electron is $9 \times 10^{-28} \ g$):

When the uncertainty in the position of a moving particle is $0$,then the uncertainty in momentum $(p)$ is equal to:

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

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