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

The work function of a metal is 6.63 × 10⁻¹⁹ J.
Calculate the maximum wavelength of the photon required to
just eject a photoelectron from the metal.
(Nearest integer in nm)

Given:
h = 6.63 × 10⁻³⁴ J s
c = 3 × 10⁸ m/s

The de Broglie wavelength of an electron and a neutron become equal when the velocity of the electron is x times the velocity of the neutron. The value of x is:

[Given:  Mass of electron is \(9.1 \times 10^{-31} \text {kg}\) and mass of neutron is \( 1.6 \times 10^{-27} \mathrm{~kg} \)]