Uncertainty in the position of an electron $\left( {{\rm{mass}} = 9.1 \times {{10}^{ - 31}}{\rm{kg}}} \right)$ moving with a velocity 300 ${\rm{m}}{{\rm{s}}^{ - 1}}$ accurate upon 0.001% will be $\left( {h = 6.63 \times {{10}^{ - 34}}{\rm{\;Js}}} \right)$

$1.92 \times {10^{ - 2}}{\rm{m}}$

$19.2 \times {10^{ - 2}}{\rm{m}}$

$5.76 \times {10^{ - 2}}{\rm{m}}$

$3.84 \times {10^{ - 2}}{\rm{m}}$

NEET UG CHEMISTRY MCQ: STRUCTURE OF ATOM

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Uncertainty in the position of an electron

\left( {\mathrm{mass} = 9.1 \times {{10}^{ - 31}}\mathrm{kg}} \right)

moving with a velocity 300

\mathrm{m}{\mathrm{s}^{ - 1}}

accurate upon 0.001% will be

\left( {h = 6.63 \times {{10}^{ - 34}}\mathrm{\;Js}} \right)

View answer and explanation

Correct option: C

1.92 \times {10^{ - 2}}\mathrm{m}

Option D (91.2 nm) is correct because it is calculated using the formula λ = hc/E, where E is the ionization potential.

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