Question

1. What is the wavelength, in nanometers, of light with a frequency of 1.25×10¹⁵ Hz? ________nm

2. Some chemical reactions, such as formation of ozone in Earth’s stratosphere, can be initiated by light that has a wavelength less than some particular value.

Calculate the longest wavelength (nm) that can provide an energy of at least 374 kJ/mol. _______ nm

3.An energy of 6.8 X 10^-19 J/atom is required to cause an aluminum atom on a metal surface to lose an electron.

Calculate the longest possible wavelength of light that can ionize an aluminum atom. ______

4. Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to fade and your skin to develop a sunburn. If you are bombarded with 1.00 mol of photons with a wavelength of 335 nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to?

Energy = ______ kJ/mol

Answer 1