Determine the energy of 2.00 mol of photons for each of the following kinds of light. (assume three significant figures.) you may want to reference (pages 299 - 308) section 7.2 while completing this problem. part a infrared radiation (1460 nm )

The energy of 2.00 mol of photons of an infrared radiation 1460 nm is 164.08 kilo Joules.

Explanation:

where,

E = energy of a photon = ?

h = Planck's constant =

c = speed of light =

= wavelength =

Now put all the given values in the above formula, we get the energy of the photons.

1 mol = particles

Then in 2 moles of photons have:

photons

Total energy of the photons = E'

The energy of 2.00 mol of photons of an infrared radiation 1460 nm is 164.08 kilo Joules.

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.

increased stability in the completion of fluorine's outer shell.