Question

6. What is the wavelength, in nm, associated with a photon of energy of 4.36 x 10-18 J? (4.56 x 101 nm)

The numbers in parenthesis is the answer that the teacher gave but I on't know how to get there. Help please!

Answer 1

Step-by-step explanation:

λ = hc/E

6.626 x 10^-34 J-s x 2.998 x 10^8 m-s^-1

4.36 x 10^-18 J

= 4556.13486239

= 4.56 x 10^1 nm

Answer 2

Step-by-step explanation:

h= e/v

6.022 x 10^23 = 4.36 x 10^-18/ v

v= 6.58 x 10^15

C= lambda x frequency

3.00 x 10^8= 6.58 x 10^15 x lambda

lambda (y)= 4.56 x 10^-8