To solve this problem, we need to use the equation that relates energy, wavelength and Planck's constant:

E = h * c / λ

where:
E is the energy,
h is Planck's constant (6.626 x 10^-34 Js),
c is the speed of light (3.00 x 10^8 m/s), and
λ is the wavelength.

We are given the energy in kJ/mol, but we need it in Joules per photon. To convert, we use Avogadro's number (6.022 x 10^23 mol^-1):

E = 146. kJ/mol * (1 mol / 6.022 x 10^23 photons) * (1000 J / 1 kJ) = 2.42 x 10^-19 J/photon

Now we can solve for λ:

λ = h * c / E
λ = (6.626 x 10^-34 Js) * (3.00 x 10^8 m/s) / 2.42 x 10^-19 J/photon
λ = 8.20 x 10^-7 m

So, the maximum wavelength of light for which an oxygen-oxygen single bond could be broken by absorbing a single photon is 8.20 x 10^-7 m, or 820 nm.

Question

To solve this problem, we need to use the equation that relates energy, wavelength and Planck's constant:

E = h * c / λ

where:
E is the energy,
h is Planck's constant (6.626 x 10^-34 Js),
c is the speed of light (3.00 x 10^8 m/s), and
λ is the wavelength.

We are given the energy in kJ/mol, but we need it in Joules per photon. To convert, we use Avogadro's number (6.022 x 10^23 mol^-1):

E = 146. kJ/mol * (1 mol / 6.022 x 10^23 photons) * (1000 J / 1 kJ) = 2.42 x 10^-19 J/photon

Now we can solve for λ:

λ = h * c / E
λ = (6.626 x 10^-34 Js) * (3.00 x 10^8 m/s) / 2.42 x 10^-19 J/photon
λ = 8.20 x 10^-7 m

So, the maximum wavelength of light for which an oxygen-oxygen single bond could be broken by absorbing a single photon is 8.20 x 10^-7 m, or 820 nm.

Knowee AI · Accepted Answer