Calculate the wavelength of light required to ionize a sodium ion.?

Question

Calculate the maximum wavelength, in nm. IE of Na+ is 4560 Kj/mole

Answer 1

Energy required to ionise Na to Na+ = 4560 kJ/mol = 4560 x 1000 J/mol
Now,we know that energy due to a wave = hv, where h is the planck's constant and v is the frequency of radiation.
vb = c (b= wavelength of radiation, c=speed of light=3 x 10^8 m/s)
Therefore,
E = hc/b
E= 4560000 J/mol
h= 6.626 x 10^-34 Js
c = 3 x 10^8 m/s
b = hc/E
substituting the values:
b= 6.626 x 10^-34 Js x 3 x 10^8 m/s / 4560000 J/mol
= 4.359 x 10^-32 m/mol
= 4.359 x 10^-32 x 6.022 x 10^23 m
= 2.62 x 10^-8 m ≈ 262 nm

Answer 2

remember that a million mole = 6.02 * 10^23 So the quantity of potential mandatory to break one bond is 338 * 10^3 / 6.02 * 10^23 J From the Einstein/Plank relation, the flexibility of a quantum is given via E = h f = h / ? h = Planks consistent (Js); ? = wavelength (m) So ? = h / E = 6.sixty seven * 10^-34 * 6.02 * 10^23 / 338 * 10*3 m ? = 0.119 * 10^ -14 = a million.19 * 10^-thirteen m, to 3 significant figures.

Answer 3

use equation E=n*h*wavelength
where n= number of atoms
h= planks constant = 6.3 x 10^(-34) Js

now put E as 4560
n 6.023 * 10^(-23)

calculate wavelength