Question

Assuming an ionization efficiency of 13.0%, how many such photons are needed to ionize 1.00×1016 atoms?

Answer 1

7.69x
`10^(16)`

Step-by-step explanation:

The ionization is the energy necessary to transform an atom in an anion. So, it's the energy it requires to gain an electron.

This ionization occurs for the photoelectric effect - the emission of electrons by metal using photons. So, if the efficiency is 100%, 1 photon can ionize 1 atom, but for an effficiency of 13.0%:

N =
`(1.00x10^(16))/(0.13)`

N = 7.69x
`10^(16)`

Where N is the number of photons.