Question

What is the wavelength, in nm, of radiation which has an energy if 3.371 x 10^-19 joules per photon?

A) 655.9nm
B)152.5nm
C)170.0nm
D) 589.3nm
E)745.1nm
Explain please

Answer 1

The correct option is:

D) 589.3 nm

Step-by-step explanation:

Energy of one photon =
`3.371*10^(-19)J`

`Energy=(hc)/(\lambda)\\\\h=Planck's\:constant=6.626*10^(-34)J/s\\c=speed\:of\:light=3*10^(8)m/s\\\lambda=wavelength\:of\:radiation\\\\\lambda=(hc)/(Energy)=(6.626*10^(-34)*3*10^(8))/(3.371*10^(-19))=5.897*10^(-7)m=589.7nm\\`

Hence, the wavelength (in nm) of radiation is 589.7nm (approximately equal to 589.3nm)