Sodium vapour lamps used for public lighting emitting 589 nm yellow light. Calculate the energy emitted by: an excited atom when it generates a photon at this wavelength and calculate the energy emitted by 0.1mol of excited Sodium atom at this wave length?
You may want to spell chemistry right.
E = hc/wavelength
for one atom.
That x 6.02E22 atoms for 0.1 mol.
To calculate the energy emitted by an excited sodium atom when it generates a photon at the wavelength of 589 nm, we can use the equation:
E = hc/λ
Where E is the energy of the photon, h is the Planck's constant (6.626 x 10^-34 J.s), c is the speed of light (3.00 x 10^8 m/s), and λ is the wavelength of the photon.
Substituting the given values:
E = (6.626 x 10^-34 J.s * 3.00 x 10^8 m/s) / (589 x 10^-9 m)
E = 3.37 x 10^-19 J
The energy emitted by an excited sodium atom when it generates a photon at 589 nm is approximately 3.37 x 10^-19 J.
To calculate the energy emitted by 0.1 mol of excited sodium atoms at this wavelength, we need to multiply the energy of a single atom by Avogadro's number (6.022 x 10^23 atoms/mol) and then multiply by the number of moles:
Energy emitted by 0.1 mol of excited sodium atoms = 0.1 mol * (6.022 x 10^23 atoms/mol) * (3.37 x 10^-19 J/atom)
Energy emitted by 0.1 mol of excited sodium atoms = 2.02 x 10^5 J
Therefore, the energy emitted by 0.1 mol of excited sodium atoms at the wavelength of 589 nm is approximately 2.02 x 10^5 J.