The approximate mass of an electron is $10^{- 27}$ . Calculate the uncertainty in its velocity if the uncertainty in its position were of the order of $10^{- 11}$ m.
$(h = 6.6 \times 10^{- 34} k g m^{2} s e c^{- 1})$

5.25 \times 10^{7}

s^{- 1}

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5.25 \times 10^{8}

s^{- 1}

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5.25 \times 10^{3}

s^{- 1}

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5.25 \times 10^{9}

s^{- 1}

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Solution

The correct option is C $5.25 \times 10^{3}$ m $s^{- 1}$
$Δ x (m . Δ v) = h / 4 π$ here $Δ v$ = uncertainty in velocity
$10^{- 11} \times 10^{- 27} \times Δ v = 6.626 \times$ $10^{- 34} / 4 \times 22 / 7$
$= 5.25 \times 10^{3} m s^{- 1}$

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The approximate mass of an electron is 10−27. Calculate the uncertainty in its velocity if the uncertainty in its position were of the order of 10−11m. (h=6.6×10−34kgm2sec−1)

The correct option is C 5.25×103 m s−1Δx(m.Δv)=h/4π here Δv = uncertainty in velocity10−11×10−27×Δv=6.626×10−34/4×22/7 =5.25×103ms−1

The approximate mass of an electron is $10^{- 27}$ . Calculate the uncertainty in its velocity if the uncertainty in its position were of the order of $10^{- 11}$ m.
$(h = 6.6 \times 10^{- 34} k g m^{2} s e c^{- 1})$

The correct option is C $5.25 \times 10^{3}$ m $s^{- 1}$
$Δ x (m . Δ v) = h / 4 π$ here $Δ v$ = uncertainty in velocity
$10^{- 11} \times 10^{- 27} \times Δ v = 6.626 \times$ $10^{- 34} / 4 \times 22 / 7$
$= 5.25 \times 10^{3} m s^{- 1}$