g It takes to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon. Round your answer to significant digits.

The maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is 349 nm.

Note: The question is incomplete. The complete question is given below:

It takes 348./kJmol to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon.

Round your answer to 3 significant digits.

Explanation:

From the question, it takes 348 kJ/mol to break a carbon-carbon triple bond.

Thus, the energy required to break 1 mole of carbon-carbon triple bond = 348 kJ = 348,000 J/mol.

For a single carbon-carbon single bond, energy required is given as E.

E = Energy required per mol/number of atoms per mole, NA

NA = 6.02 × 10²³

E = 348000 J / 6.02 × 10²³ = 5.7 × 10-¹⁹ J

This energy will be equivalent to the wavelength of the photon of light absorbed by the atom.

From Planck's equation, E = hc/λ

Where c = velocity of light = 3.0 × 10⁸ m/s

h is Planck's constant = 6.63 × 10-³⁴ Js

λ is wavelength of photon

Making λ subject of the formula:

λ = hc/E

λ = (6.63 × 10-³⁴ Js × 3.0 × 10⁸ m/s)/5.7 × 10-¹⁹ J

λ = 3.49 × 10-⁷m = 349 nm

The maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is 349 nm.

can you attach the