What is the de Broglie wavelength of an electron traveling at 1.35 x 10^5 m/s?

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1. Identify the formula for the de Broglie wavelength: $\lambda =\frac{h}{mv}$, where $\lambda$ is the wavelength, $h$ is Planck's constant (6.626 x 10^{-34} \text{ m}^2 \text{ kg/s}), $m$ is the mass of the electron (9.109 x 10^{-31} \text{ kg}), and $v$ is the velocity of the electron.
2. Substitute the given velocity $v=1.35\times {10}^5\text{ m/s}$ into the formula.
3. Substitute the known values for Planck's constant $h=6.626\times {10}^{-34}{\text{ m}}^2\text{ kg/s}$ and the mass of the electron $m=9.109\times {10}^{-31}\text{ kg}$ into the formula.
4. Calculate the de Broglie wavelength by performing the division $\lambda =\frac{6.626\times {10}^{-34}}{9.109\times {10}^{-31}\times 1.35\times {10}^5}$.
5. Simplify the expression to find the de Broglie wavelength $\lambda$.