What is the de Broglie wavelength of an electron traveling at 1.26×105m/s ?
wavelength = h/mv
m = mass in kg
v = velocity in m/s
6.626 x 10^-34/ m x 1.26 times 10^5
what is plugged in for the mass if it is not given?
To find the de Broglie wavelength of an electron, we can use the de Broglie wavelength formula:
λ = h / p,
where λ is the de Broglie wavelength, h is the Planck's constant (6.626 x 10^-34 J·s), and p is the momentum of the electron.
The momentum (p) of an electron can be calculated using the formula:
p = m * v,
where m is the mass of the electron (9.10938356 x 10^-31 kg) and v is the velocity of the electron.
Now we can substitute the given values into the formulas to find the de Broglie wavelength.
First, let's calculate the momentum:
p = (9.10938356 x 10^-31 kg) * (1.26 x 10^5 m/s)
p ≈ 1.1511 x 10^-24 kg·m/s
Now we can use the momentum to calculate the de Broglie wavelength:
λ = (6.626 x 10^-34 J·s) / (1.1511 x 10^-24 kg·m/s)
λ ≈ 5.749 x 10^-10 m
Therefore, the de Broglie wavelength of an electron traveling at 1.26×10^5 m/s is approximately 5.749 x 10^-10 meters.