(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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$A$ 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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The uncertainty in the location of a circulating electron is equal to its de Broglie wavelength. The minimum percent error in its measurement of velocity under these circumstances will be approximately:

The electrons are more likely to be found

The uncertainty in the position of a particle of mass $0.25 \, kg$ is $10^{-5} \, m$. The uncertainty in its velocity is ...... $m/s$.

An electron is moving with a velocity of $600 \, m/s$ with an accuracy of $0.005\%$. The uncertainty in its position will be: ($h = 6.6 \times 10^{-34} \, kg \, m^2 \, s^{-1}$,mass of electron $m_e = 9.1 \times 10^{-31} \, kg$)

The correct form of the $Schrodinger$ wave equation for an electron,as derived by $Erwin$ $Schrodinger$,is:

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