Question

Calculate the energy of one mole of photon of radiation whose frequency is 5×10^14 Hz..

Answer 1

E=hv(nu)
E=6.626×10^-34×5×10^14 =33.13×10^-20
E=33.13×10^-20×6.022×10^23. =199.50×10^-3

Answer 2

Answer: The energy of one mole of photon of radiation is, $23.851\times 10^{-17}J$

Explanation:

A mole is defined as the amount of substance that contains Avogardro number of the substance. Avogadro's number is given by $6.022\times 10^{23}$.

Energy for 1 photon is given by:

$E=\frac{hc}{\lambda}$

Energy for 1 mole photon is given by:

$E=\frac{N_Ahc}{\lambda}$

$N_A$ = avogadro's no

E= energy

h= planks constant =$6.6\times 10^{-34}J/s$

c = speed of light = $3\times 10^8m/s$

$\lambda$ = Wavelength of radiation  = $5\times 10^{14}Hz$

Puting in the values:

$E=\frac{6.023\times 10^{23}\times 6.6\times 10^{-34}\times 3\times 10^8}{5\times 10^{14}}=23.851\times 10^{-17}J$

Therefore, the energy of one mole of photon of radiation is, $23.851\times 10^{-17}J$