A gas absorbs a photon of 355 nm and emits at two wavelengths. If one of the emissions is at 680 nm, the other is at:

1. 1035 nm

2. 325 nm

3. 743 nm

4. 518 nm

The energy required to break one mole of CI–Cl bonds in Cl₂ is 242 kJmol⁻¹. The wavelength of light capable of breaking a single Cl–Cl bond is:$\mathrm{}\mathrm{}\mathrm{}{\mathrm{}}^{\mathrm{}}{}^{\mathrm{}}{\mathrm{}}_{\mathrm{}}$

1. 494 nm

2. 594 nm

3. 640 nm

4. 700 nm