Unleash Your Physics Knowledge: Calculate the Wavelength of an Electron!

What is the wavelength of an electron with a kinetic energy of 1.23*10 to the power of 6 J/mol?

Option 1: 8.362*10 to the power of -11 m

Option 2: 4.5658*10 to the power of -14 m

Option 3: 1.092*10 to the power of -11 m

Option 4: 2.5598*10 to the power of -13 m

Option 5: None of the above

Answer:

The wavelength of an electron with a kinetic energy of 1.23*10^6 J/mol is 4.579 x 10^-12 m.

Let's dive into the exciting world of physics! The de Broglie equation helps us calculate the wavelength of particles like electrons. In this case, we have an electron with a kinetic energy of 1.23*10^6 J/mol.

We can use the de Broglie equation:

λ = h / p

Where λ is the wavelength, h is Planck's constant (6.626 x 10-34 J s), and p is the momentum of the electron. To find the momentum, we can use the equation:

p = √(2mE)

Plugging in the values, we get:

p = √ (2 * 9.11 x 10-31 kg * 1.23 x 106 J/mol)

p = 1.44 x 10-22 kg m/s

Now, we can calculate the wavelength:

λ = (6.626 x 10-34 J s) / (1.44 x 10-22 kg m/s)

Which gives us a wavelength of 4.579 x 10-12 m.

Physics is truly fascinating! By understanding the principles and equations, we can unlock the mysteries of the universe. Keep exploring and expanding your knowledge!