divide the energy by 2*avagrado's number, the number of atoms in a mole of H2
Then, use Planck's equation to find the wavelength.
They give the equation E=hcR but those are all known constant values and none include mols so I'm very confused.
Thanks!
Then, use Planck's equation to find the wavelength.
So my answer should be 182.45 nm, yes?
So I did:
1312200/2(6.022x10^23)
6.626x10^-34(3x10^8)/ans
and then that answerx 10^9 to convert to nm
Where did I go wrong because that answer wasn't correct =(
http://en.wikipedia.org/wiki/Molar_ionization_energies_of_the_elements
This shows ionization energy = 1312 kJ/mol H ATOMS.
First, let's convert the given ionization energy from kJ/mol to J/atom. Since there are Avogadro's number (6.022 × 10^23) of atoms in one mole, we can divide the ionization energy by Avogadro's number to get the energy per atom.
1312.2 kJ/mol = (1312.2 × 10^3 J/mol) ÷ (6.022 × 10^23 atoms/mol) ≈ 2.182 × 10^-18 J/atom
Now, we can substitute this energy value into the equation to find the wavelength (λ).
2.182 × 10^-18 J/atom = (6.626 × 10^-34 J·s) × (2.998 × 10^8 m/s) ÷ λ
Rearranging the equation and solving for λ:
λ = (6.626 × 10^-34 J·s) × (2.998 × 10^8 m/s) ÷ (2.182 × 10^-18 J/atom)
Calculating this expression:
λ ≈ 9.104 × 10^-8 m
Finally, to convert the wavelength from meters (m) to nanometers (nm), we multiply by 10^9:
λ ≈ 9.104 × 10^-8 m × 10^9 nm/m ≈ 91.04 nm
Therefore, the wavelength of a photon with enough energy to ionize one atom of hydrogen is approximately 91.04 nm.