undergoes photochemical dissociation into one normal oxygen atom and one oxygen atom 1.2 eV more energetic than normal. The dissociation of into two normal atoms of oxygen requires 482.5 kJ/mol. The

Question

undergoes photochemical dissociation into one normal oxygen atom and one oxygen atom 1.2 eV more energetic than normal. The dissociation of  into two normal atoms of oxygen requires 482.5 kJ/mol. The maximum wavelength effective for photochemical dissociation of  is (1 eV = 96.5 kJ/mol)

Canvas Classes · Accepted Answer

Step 1: Energy needed for photochemical dissociation

The photon must provide energy to:
1. Dissociate  into two normal O atoms:  kJ/mol
2. Give one O atom an extra  eV of energy

Converting 482.5 kJ/mol to eV:

Total energy needed:

Step 2: Maximum wavelength

Maximum wavelength corresponds to minimum energy (= exactly 6.2 eV):

(Using  eV·nm)

Final Answer: 200 nm → Option (d)

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