Question

calculate the energy of a mole of photons of radiation whose frequency is 5×10^14 Hz​

Answer 1

Answer:

frequency of radiation=5x10^14

planks constant =6.626x10^-34

energy=frequency x planks constant

$energy = 5 \times 10 {}^{14} \times 6.626 \times 10 \times {}^{ - 34}$

$energy \: of \: photons = 33.13 \times 10 {}^{ - 20}$

Answer 2

Answer:

The energy of a mole of photons of radiation whose frequency is 5×10^14 Hz​ is $198.6*10^{3}J$

Explanation:

• The quantum theory of radiation, gives the photon energy is quantized

• For radiation of frequency (ν) the energy (E) is given as

       $E=nh$ν

       where,

       n-number of photons

       $h=6.6*10^{-34} Js$-Planck's constant

From the question, we have

frequency of the radiation ν $=5*10^{14} Hz$

number of photons in one mole of photos is Avogadro number, that is $6.02*10^{23}$ photos

the energy of the radiation $E=6.02*10^{23}*6.6*10^{-34}*5*10^{14} =198.6*10^{3}J$