using balmer series calculate ionisation energy of hydrogen atom in kJmol -1
Answers
The Balmer series is the description for the spectral lines of emissions from the hydrogen atom
The initial energy state is 1 .
Multiply Rydberg constant 1.097 x 10^(7) per meter (1/m). This gives the original Rydberg constant.
Calculate the inverse of result A (This gives 9.11 x 10^(-8) m. This is the wavelength of the spectral emission.
Multiply Planck's constant by the speed of light, and divide the outcome by the wavelength of the emission. Multiplying Planck's constant, which has a value of 6.626 x 10^(-34) Joule seconds (J s) by the speed of light, which has a value of 3.00 x 10^8 meters per second (m/s) gives 1.988 x 10^(-25) Joule meters (J m), and dividing this by the wavelength (which has a value of 9.11 x 10^(-8) m) gives 2.182 x 10^(-18) J. This is the first ionization energy of the hydrogen atom.
Multiply the ionization energy by Avogadro's number, which gives the number of particles in a mole of substance. Multiplying 2.182 x 10^(-18) J by 6.022 x 10^(23) gives 1.312 x 10^6 Joules per mol (J/mol), or 1312 kJ/mol, which is how it is normally printed in chemistry.