Question

it takes 348 kj/mol to break 1 mole of c-c bonds. what would be the minimum frequency of a photon needed that could break a single (1) c-c bond?

Answer 1

The minimum frequency of a photon needed to break a single C-C bond is approximately 8.73 x 10^14 Hz.

Step-by-step explanation:

To determine the minimum frequency of a photon needed to break a single C-C bond, we need to convert the bond energy value given in kJ/mol to J/molecule. We can then use the equation E = hν to calculate the minimum frequency (h is Planck's constant) using the energy value we just obtained. Let's proceed with the calculations:

Given: Energy to break 1 mole of C-C bonds = 348 kJ/mol

1 mole = 6.022 x 1023 molecules (Avogadro's number)

First, let's convert 348 kJ/mol to J/molecule:

348 kJ/mol x 1000 J/1 kJ x 1 mol/6.022 x 1023 molecules ≈ 5.78 x 10-19 J/molecule

Now we can use this energy value to calculate the minimum frequency:

E = hν

5.78 x 10-19 J/molecule = h x ν

ν = (5.78 x 10-19 J/molecule) / h

Planck's constant, h = 6.626 x 10-34 J·s

Calculating the minimum frequency:

ν = (5.78 x 10-19 J/molecule) / (6.626 x 10-34 J·s) ≈ 8.73 x 1014 Hz

Therefore, the minimum frequency of a photon needed to break a single C-C bond is approximately 8.73 x 1014 Hz.