Calculate the energy (in kJ/mol) of each of the following photons given either the frequency or the wavelength: 1.60×10¹⁴ s⁻¹, 2.34×10¹⁴ s⁻¹, and 1.09×10⁻⁶ m.

One watt (W) is equal to 1 J/s. How many photons are released by a light bulb every second if 4.5% of the energy produced by a 55 W light bulb is visible light and its average wavelength is 530 nm?

The photodissociation of ozone happens in the troposphere: 

O₃ + hν → O₂ + O 

A light with a maximum wavelength of 320 nm can initiate this reaction. Calculate the maximum bond strength (kJ/mol) that can be broken by the absorption of 320 nm light.

What is the effect of greenhouse gases on how the planet cools given that the sun provides average energy of 168 watts per square meter while the Earth's surface emits an average of 390 watts per square meter?

Calculate the percent efficiency for the conversion of power to light for a certain LED light that uses 144.0 watts of electrical power to emit 1.27×10²⁰ 535-nm photons per second.

Calculate the energy (kJ) of 2.50 moles of photons for radiation with a wavelength of 295 nm within the UV region.

The laser pointer emits light because electrons in the material are excited (by a battery) from their ground state to an upper excited state. When the electrons return to the ground state, they lose the excess energy in the form of 532-nm photons. What is the energy gap between the ground state and the excited state in the laser material?