Complete the exercises below. a. If a complex absorbs light at 610 nm, what color would you expect the complex to be? b. What is the energy in joules of a photon with a wavelength of 610 nm? c. What is the energy of this absorption in kJ/mol?

Verified step by step guidance

1. Step 1: To determine the color of the complex, first understand that the color observed is complementary to the color absorbed. Use the color wheel to find the complementary color of 610 nm, which is in the orange-red region.
2. Step 2: To find the energy of a photon with a wavelength of 610 nm, use the equation E = \frac{hc}{\lambda}, where h is Planck's constant (6.626 \times 10^{-34} \text{ J s}), c is the speed of light (3.00 \times 10^8 \text{ m/s}), and \lambda is the wavelength in meters.
3. Step 3: Convert the wavelength from nanometers to meters by using the conversion factor 1 nm = 1 \times 10^{-9} m.
4. Step 4: Calculate the energy of one photon in joules using the values from Step 2 and the converted wavelength from Step 3.
5. Step 5: To find the energy in kJ/mol, multiply the energy of one photon by Avogadro's number (6.022 \times 10^{23} \text{ mol}^{-1}) and convert the result from joules to kilojoules by dividing by 1000.