Please Help! How much energy is contained in 1 mol of each of the following?

Convert wavelength (l) to frequency (v) by using

c = vl or v = c/l where c is the speed of light (3x10^8 m/s).

Then use E (energy) = hv where h is equal to Planck's constant. You can look up Planck's constant on the front cover of your chemistry or physics textbook.

The E that you calculate is for one photon. To calculate for a mole of photons, multiply by Avagadro's number, 6.02 x 10^23.

The formulas are the same for A and B. The answers will be different though because the wavelengths are different. Gamma rays will have higher energy.

Ephoton = hc/? Ephoton = (6.626*10^-34) (3.00*10^8) / (.one hundred thirty five*10^-9 meters) Ephoton = a million.40 seven*10^-15 J # of photons = a million mole = 6.022*10^23 # photons = Epulse / Ephoton 6.022*10^23 = Epulse / a million.40 seven*10^-15 J remedy for Epulse = 8.867*10^8 J Convert to kJ = 8.867*10^5 kJ comparable for gamma-ray Ephoton = (6.626*10^-34) (3.00*10^8) / (2.sixty 3*10^-5 nm *10^-9 meters) Ephoton = 7.857*10^-12 # of photons = a million mole = 6.022*10^23 # photons = Epulse / Ephoton 6.022*10^23 = Epulse / 7.857*10^-12 remedy for Epulse = (6.022*10^23) = 4.seventy 3*10^12 J Convert to kJ = 4.seventy 3*10^9 kJ