Question

a photochemical reaction requires 9.6×10^-16 J energy per molecule calculate the number of photons per molecule of light with wavelength 250 nm that is just sufficient to initiate the reaction

Answer 1

mark me

i consider that if i provide just the energy needed by one molecule that would initiate the reaction.

so the total energy that i need is 9.6x10^-16 J.

now energy carried by one photon is

E = hc/λ

E = 8* 10^-19 J

assume the total no. of photons needed is n,

nE = total energy

n( 8* 10^-19) = 9.6x10^-16

n = 1200

Answer 2

Explanation:

I'm not sure about the answer but it's most probably this only!!