Question

It takes 3.8x10-19 J to remove an electron from an atom. What is the wavelength
of the light?

Answer 1

The wavelength of the light is 523 nm

Step-by-step explanation:

Given:

i) First let us determine the frequency:

The energy required to remove an electron = 3.8 x
`10^(-19)`J

Using Planck's constant the formula for energy, E = hv

3.8 x
`10^(-19)` = (6.626 x
`10^(-34)` Js) (x)

Here Planck's constant h = 6.626 x
`10^(-34)`

x = 0.5734 x
`10^(15)`

x = 5.734 x
`10^(14)`
`s^(-1)`

ii) Secondly, let us determine the wavelength:

`\bold{\lambda v = c}`

(x) (5.734 x
`10^(14)`
`s^(-1)`) = 3 x
`10^8` m/s

Here speed of light c = 3 x
`10^8` m/s

x = 0.5231 x
`10^(-6)`

x = 5.231 x
`10^(-7)` m

x = 523 nm