Question

What quantity of energy (in kJ) is contained in a burst of gamma rays which contains 1.75 moles of photons which have a frequency of 5.80 * 1014 Hz? Can some help me solve this step by step?

Answer 1

The energy of a photon is given by this equation:
\[E = h * \nu\]
Where nu is the frequency and h is Planck's constant:
\[h = 6.626 *10^{-34} J*s\]
Therefore, the energy of each of our gamma ray photons is:
\[E = (6.626 * 10^{-34} J*s)(5.80*10^{14} s ^{-1}) = 38.4308*10^{-20} J\]
As we also know, there are 6.022e23 of anything in a mole, so we have 10.5385e23 photons. Multiplying this by the energy for one photon gives us the total energy:
\[38.4308*10^{-20} J * 10.5385*10^{23} = 405.00298*10^{3} J = 405.00298 kJ\]

Answer 2

thank you

Answer 3

Sure! Glad to help.