Calculate the de-Broglie wavelength of an electron having velocity 1000\ ^ -1 [ h = 6.626 × 10^ -34 \ js , mass of an electron = 9.1 × 10^ -31 \ kg ]

Correct answer: A. 7.28 × 10^ -7 \ m The de-Broglie wavelength is given by the formula: λ = (h)/(mv) Substituting the given values: λ = 6.626 × 10^ -34 9.1 × 10^ -31 × 1000 λ = 6.626 × 10^ -34 9.1 × 10^ -28 λ = 0.728 × 10^ -6 \ m λ = 7.28 × 10^ -7 \ m Answer: 7.28 × 10^ -7 \ m

MHT CET 202625 AprilEvening Shift

Exam: MHT CET
Year: 2026
Date: 25 April
Shift: Evening Shift
Subject: Chemistry
Chapter: Structure of Atom

MHT CET 2026 · 25 April · Evening Shift · Chemistry · Structure of Atom

Calculate the de-Broglie wavelength of an electron having velocity...

Calculate the de-Broglie wavelength of an electron having velocity

1000\ \text\mathrm\mathrm\mathrm\mathrm\mathrm\mathrm\mathrm\mathrm\mathrm\mathrm\mathrm{ms}^{-1}

[

h = 6.626 \times 10^{-34}\ \text{js}

, mass of an electron

= 9.1 \times 10^{-31}\ \text{kg}

]

Options

A $7.28 \times 10^{-7}\ \text{m}$
B $6.68 \times 10^{-7}\ \text{m}$
C $7.76 \times 10^{-7}\ \text{m}$
D $7.45 \times 10^{-7}\ \text{m}$

Correct answer

A. $7.28 \times 10^{-7}\ \text{m}$

Step-by-step solution

The de-Broglie wavelength is given by the formula:

\lambda = \dfrac{h}{mv}

Substituting the given values:

\lambda = \dfrac{6.626 \times 10^{-34}}{9.1 \times 10^{-31} \times 1000}

\lambda = \dfrac{6.626 \times 10^{-34}}{9.1 \times 10^{-28}}

\lambda = 0.728 \times 10^{-6}\ \text{m}

\lambda = 7.28 \times 10^{-7}\ \text{m}

Answer:

7.28 \times 10^{-7}\ \text{m}

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