Question

) What total energy (in kJ) is contained in 1.0 mol (6.022 × 1023) of photons, all with a frequency of 2.75 × 1014 Hz​

Answer 1

Answer -

The energy of a photon is E = h*f

where h is Planck's constant and f is the frequency of the photon.

h= 6.62607004 × 10^-34 m² kg / s

If the frequency is f = 2.75*10^14 Hz, then the energy of one photon is:
E = h * f

E= 6.62607004 × 10^-34 m² kg / s * 2.75 × 10¹⁴ Hz

E = 1.82*10^-19 J
If you want the energy of a mole of photons, multiply that energy by Avogadro's number.

The energy of one-mole photon = 6.022*10²³*1.82*10^-19 J

The energy of the one-mole photon = 10.96 *10⁴ J = 109.6 kJ