Answer:
[tex]2.46\cdot 10^5 J[/tex]
Explanation:
The enegy of a single photon is given by:
[tex]E=\frac{hc}{\lambda}[/tex]
where
h is the Planck costant
c is the speed of light
[tex]\lambda[/tex] is the wavelength of the photon
In this problem,
[tex]\lambda=486 nm=4.86\cdot 10^{-7}m[/tex]
so the energy of one photon is
[tex]E_1=\frac{(6.63\cdot 10^{-34} Js)(3\cdot 10^8 m/s)}{4.86\cdot 10^{-7}m}=4.09\cdot 10^{-19} J[/tex]
1 mole of photons contains a number of Avogadro of photons:
[tex]N_A = 6.022\cdot 10^{23}[/tex]
therefore, the total energy of 1 mole of these photons will be
[tex]E=N_A E_1 = (6.022\cdot 10^{23})(4.09\cdot 10^{-19} J)=2.46\cdot 10^5 J[/tex]
