the atomic spectrum of lithium has a strong red line at 670.8 nm. what is the energy of each photon of this wave length? What is the energy of 1 mole of these photons??
-do you use the e=h x v ??
Yes, to calculate the energy of a photon, you can use the formula E = h * ν, where E is the energy of the photon, h is Planck's constant (6.626 x 10^-34 J·s), and ν is the frequency of the photon.
However, in order to use this formula, we need to first determine the frequency of the photon using the given wavelength. The relationship between wavelength (λ) and frequency (ν) is given by the equation c = λν, where c is the speed of light (3.00 x 10^8 m/s).
To determine the frequency (ν) of the given wavelength, we can rearrange the equation c = λν:
ν = c / λ
Given that the wavelength (λ) is 670.8 nm (or 670.8 x 10^-9 m) and the speed of light (c) is 3.00 x 10^8 m/s, we can substitute these values into the equation:
ν = (3.00 x 10^8 m/s) / (670.8 x 10^-9 m)
ν ≈ 4.476 x 10^14 s^-1
Now that we have the frequency (ν), we can calculate the energy of each photon (E) using the formula E = h * ν:
E = (6.626 x 10^-34 J·s) * (4.476 x 10^14 s^-1)
E ≈ 2.964 x 10^-19 J
To calculate the energy of 1 mole of these photons, we need to multiply the energy of each photon by Avogadro's number (6.022 x 10^23 mol^-1):
Energy of 1 mole of photons = (2.964 x 10^-19 J) * (6.022 x 10^23 mol^-1)
Energy of 1 mole of photons ≈ 1.785 x 10^5 J/mol
Yes, to find the energy of each photon, you can use the equation E = h x v, where E represents energy, h is Planck's constant (6.63 x 10^-34 J*s), and v is the frequency of the photon. However, in this case, we are given the wavelength (λ) of the photon rather than the frequency. To find the frequency, we can use the equation v = c/λ, where c is the speed of light (3.00 x 10^8 m/s).
First, let's calculate the frequency:
v = c/λ
v = (3.00 x 10^8 m/s) / (670.8 x 10^-9 m)
v ≈ 4.47 x 10^14 Hz
Now that we have the frequency, we can calculate the energy of each photon:
E = h x v
E = (6.63 x 10^-34 J*s) * (4.47 x 10^14 Hz)
E ≈ 2.967 x 10^-19 J
To find the energy of 1 mole of these photons, we can multiply the energy of each photon by Avogadro's number (6.022 x 10^23 photons/mol):
Energy of 1 mole of photons = (2.967 x 10^-19 J/photon) * (6.022 x 10^23 photons/mol)
Energy of 1 mole of photons ≈ 1.784 x 10^5 J/mol
yes, but they give you the wavelength
e = h c / λ
make sure your units are consistent