Quiz-1

Compare the energy (in joules) carried by an x-ray photon (wavelength = 0.20 nm) with that carried by an AM radio wave photon ( wavelength = 200m). Calculate the energy of 1.00 mole of each type of photon. What effect do you expect each type of radiation to have in terms of inducing chemical reactions in the substances through which it passes?

frenquency = c / wavelength

E= hc/wavelength

1 photon

Ex-ray = 6.63*10^-34(js) * 2.99*10^8(m/s) / 0.20 *10^-9m = 9.91*10^-12joules

EAM = 6.63*10^-34(js) * 2.99*10^8(m/s) / 200m = 9.91* 10^-28joules

1mole of photons

E=E1-photon * NA

Ex-ray = 9.91*10^-12j *6.02*10^23/mol = 5.97 *10^8 joules/mol

EAM = 9.91*10^-28j *6.02*10^23/mol = 5.97 *10^-4 joules/mol

Ex-ray > EAM

X-ray photon will be expected to induce chemical reactions since it has much higher energy whereas AM radio photons will not.