[Bjc51192]

Determine the energy of 2.00  of photons for each of the following kinds of light. (Assume three significant figures.)

infrared radiation (1600 ) they want the answer in kj

Ok I dont understand what my problem is much help would be appreciated.
 
Im setting up the problem like this E=hc/wavelength

E=(6.626*10^-34)*(3.00*10^8)/1600*10^-9m

You are left with 1.24*10^-28 j

I convert j to kj and get 1.24*10^-31

then I have to get the mol which means multiply by 6.022*10^23/2.00 however, the answer im getting is incorrect.

Or maybe im missing a step?

[Schrödinger]

E=(6.626*10^-34)*(3.00*10^8)/1600*10^-9m

You are left with 1.24*10^-28 j

I convert j to kj and get 1.24*10^-31

All fine upto this point. This is the energy that is contained in ONE photon.

Determine the energy of 2.00  of photons for each of the following kinds of light. (Assume three significant figures.)

Although your post doesn't say so (probably a typo), I assume that the question asks you to find the energy of 2 mol of photons.

In that case,

then I have to get the mol which means multiply by 6.022*10^23/2.00 however, the answer im getting is incorrect.

is wrong. You should be multiplying by a factor of (6.022*10^23)*2.00. You shouldn't divide by 2, because, if one mole contains 6.022*10^23 photons, then 2 moles should contain 2* 6.022*10^23 photons

[Bjc51192]

That was crystal clear. Thank you so much