I am curious if someone could check these answers for me? I believe they turned out incorrect and am curious to see what I need to do to fix them. Thanks! 1. **Light emitted by sodium vapor lamps** (like those on highway 30 outside BHS) has a wavelength (\(\lambda\)) of \(5.89 \times 10^2\) nm. a) **Calculate the frequency of this radiation in Hz.** \[ \nu = \frac{c}{\lambda} \rightarrow \frac{2.998 \times 10^8 \, \text{m/s}}{5.98 \times 10^{-7} \, \text{m}} = 5.01 \times 10^{14} \, \text{Hz} \] The frequency is \(5.01 \times 10^{14} \, \text{Hz}\). b) **Determine the energy in joules (J) of one photon of this radiation.** \[ E_{\text{photon}} = 5.01 \times 10^{14} \, \text{s}^{-1} \times 6.626 \times 10^{-34} \, \text{J}\cdot\text{s} = 3.32 \times 10^{-19} \, \text{J} \] The energy is \(3.32 \times 10^{-19} \, \text{J}\). c) **Determine the energy in joules (J) of one mole of photons which have this wavelength.** \[ \frac{3.32 \times 10^{-19} \, \text{J}}{\text{photon}} \times \frac{6.022 \times 10^{23} \, \text{photons}}{1 \, \text{mole}} = 1.99 \times 10^5 \, \text{J} \] The energy is \(1.99 \times 10^5 \, \text{J}\). d) **In what region of the light spectrum (IR, UV, visible, x-ray etc.) is this radiation found?** The text does not include a specific answer for this part, but given the wavelength of approximately \(589\) nm, it is in the visible spectrum.

To calculate the frequency of the radiation the value of C and the wavelength of the radiation should be known. Given: C=3⨉108m/s Using the formula given below we can calculate the frequency of the radiation, Frequency of the radiation is 5.0934⨉1014Hz. b) To calculate the energy of the photon of the corresponding radiation the following formula is used, Or Energy of one photon of the radiation is 3.3748⨉10-19J. c) Energy of one mole of photon of the radiation given is calculated as follows: Energy of 1 mole of the photon of the radiation is 20.32⨉104J.