Calculate the wavelength of light emitted from a mol of photons as they transition from in the hydrogen atom.

The question is incomplete, here is the complete question:

How do you calculate the wavelength of the light emitted from a mole of photons as they transition from the n = 4 to the n = 1 principal energy level in the hydrogen atom. Recall that for hydrogen

The wavelength of 1 mole of photons for the given transition is

Explanation:

To calculate the change in energy, we use the equation:

Or,

where,

= initial energy level = 4

= final energy level = 1

Putting values in above equation, we get:

To calculate the wavelength of light for 1 mole of photons, we use the equation:

where,

= Avogadro's number =

h = Planck's constant =

c = speed of light =

= wavelength of light = ?

E = energy emitted =  

Putting values in above equation, we get:

Hence, the wavelength of 1 mole of photons for the given transition is

number of molecules / avogadro's number * molecule molecular = mass

explanation:

we define a gram-molecular weight as the mass of one mole of any element or compound. a mole contains avogadro's number of units (molecules) –  

6.022

x

10

23

. so, dividing the number of molecules by avogadro's number gives us the number of moles. multiplying that by the molecular weight gives us the mass. from the periodic table we find the gram-molecular weight of u to be238 and of f to be19. so,  

u

f

6

will have a gram-molecular weight of 352g.

i think that the answer is c