What is the energy of a photon with a frequency of 3.5 X 10ˆ15 sˆ-1 in J/photon? In J/mol?
E = hf
E in joules.
h = Planck's constant
f = frequency in Hz
To calculate the energy of a photon, you can use the equation:
E = hf
where E is the energy of the photon, h is the Planck's constant (6.626 x 10^-34 J*s), and f is the frequency of the photon.
Given that the frequency of the photon is 3.5 x 10^15 s^-1, we can substitute this value into the equation to find the energy of the photon.
E = (6.626 x 10^-34 J*s) * (3.5 x 10^15 s^-1)
E = 23.141 x 10^-19 J
Therefore, the energy of a single photon with a frequency of 3.5 x 10^15 s^-1 is approximately 2.3141 x 10^-18 J/photon.
To convert this value to J/mol, we need to multiply it by Avogadro's number (6.022 x 10^23 mol^-1).
E (J/mol) = (2.3141 x 10^-18 J/photon) * (6.022 x 10^23 mol^-1)
E (J/mol) = 1.392 x 10^6 J/mol
Therefore, the energy of a mole of photons with a frequency of 3.5 x 10^15 s^-1 is approximately 1.392 x 10^6 J/mol.
To determine the energy of a photon, you can use the equation E = hν, where E represents energy, h is Planck's constant (6.626 x 10^-34 J·s), and ν (nu) represents the frequency of the photon.
1. To find the energy of a single photon (in J/photon):
E = hν
E = (6.626 x 10^-34 J·s)(3.5 x 10^15 s^-1)
E ≈ 2.314 x 10^-18 J/photon
So, the energy of a photon with a frequency of 3.5 x 10^15 s^-1 is approximately 2.314 x 10^-18 J/photon.
2. To convert this energy to J/mol, you need to multiply the energy by Avogadro's constant (6.022 x 10^23 mol^-1). This conversion is necessary because one mole contains Avogadro's number of particles (atoms, molecules, or photons).
E (J/mol) = E (J/photon) × Avogadro's constant
E (J/mol) = (2.314 x 10^-18 J/photon)(6.022 x 10^23 mol^-1)
E (J/mol) ≈ 1.393 x 10^6 J/mol
Therefore, the energy of a photon with a frequency of 3.5 x 10^15 s^-1 is approximately 1.393 x 10^6 J/mol.