What is the wavelength (nm) for a photon of light with an energy of 3.20 x 10^-19 J/photon A) 621 nm B) 631 nm C) 641 nm D) 651 nm E) None of the above

Question

Quizplus · Accepted Answer

The energy of a photon can be calculated using the equation $E = \frac{hc}{\lambda}$, where $E$ is the energy of the photon in joules, $h$ is Planck's constant ($6.626 \times 10^{-34} \, \text{m}^2 \, \text{kg} / \text{s}$), $c$ is the speed of light in a vacuum ($3.00 \times 10^8 \, \text{m/s}$), and $\lambda$ is the wavelength of the photon in meters. Rearranging the equation to solve for $\lambda$, we get $\lambda = \frac{hc}{E}$. Substituting the given values and converting the wavelength from meters to nanometers (1 m = $10^9$ nm), we find the wavelength to be approximately 621 nm.

What Is the Wavelength (Nm) for a Photon of Light