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 per mole of photons,
h is 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.

First, we need to convert the energy from kJ/mol to J/photon. We know that 1 mol of photons contains Avogadro's number (6.022 x 10^23) of photons, and 1 kJ = 1000 J. So,

E = 498. kJ/mol * (1000 J/1 kJ) * (1 mol/6.022 x 10^23 photons) = 8.27 x 10^-19 J/photon

Now we can substitute E, h, and c into the equation and solve for λ:

λ = h * c / E
λ = (6.626 x 10^-34 J*s) * (3.00 x 10^8 m/s) / 8.27 x 10^-19 J/photon
λ = 2.40 x 10^-7 m

However, the wavelength of light is usually expressed in nanometers (nm), not meters. We know that 1 m = 10^9 nm, so

λ = 2.40 x 10^-7 m * (10^9 nm/1 m) = 240 nm

So, the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon is 240 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 per mole of photons,
h is 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.

First, we need to convert the energy from kJ/mol to J/photon. We know that 1 mol of photons contains Avogadro's number (6.022 x 10^23) of photons, and 1 kJ = 1000 J. So,

E = 498. kJ/mol * (1000 J/1 kJ) * (1 mol/6.022 x 10^23 photons) = 8.27 x 10^-19 J/photon

Now we can substitute E, h, and c into the equation and solve for λ:

λ = h * c / E
λ = (6.626 x 10^-34 J*s) * (3.00 x 10^8 m/s) / 8.27 x 10^-19 J/photon
λ = 2.40 x 10^-7 m

However, the wavelength of light is usually expressed in nanometers (nm), not meters. We know that 1 m = 10^9 nm, so

λ = 2.40 x 10^-7 m * (10^9 nm/1 m) = 240 nm

So, the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon is 240 nm.

Knowee AI · Accepted Answer

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 per mole of photons,
h is 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.

First, we need to convert the energy from kJ/mol to J/photon. We know that 1 mol of photons contains Avogadro's number (6.022 x 10^23) of photons, and 1 kJ = 1000 J. So,

E = 498. kJ/mol * (1000 J/1 kJ) * (1 mol/6.022 x 10^23 photons) = 8.27 x 10^-19 J/photon

Now we can substitute E, h, and c into the equation and solve for λ:

λ = h * c / E
λ = (6.626 x 10^-34 J*s) * (3.00 x 10^8 m/s) / 8.27 x 10^-19 J/photon
λ = 2.40 x 10^-7 m

However, the wavelength of light is usually expressed in nanometers (nm), not meters. We know that 1 m = 10^9 nm, so

λ = 2.40 x 10^-7 m * (10^9 nm/1 m) = 240 nm

So, the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon is 240 nm.

It takes 498./kJmol to break an oxygen-oxygen double bond. Calculate the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon.Be sure your answer has the correct number of significant digits.

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