Question

The energy of one mole of photons of radiation of wavelength \(300\) \(nm\) is (Given \(h\) = \(6.63 × 10^{–34}\)Js, \(N_A\) = \(6.02 × 10^{23}\) \(mol^{–1}\), \(c = 3 × 10^8\) \(ms^{–1}\))

• A. 235 kJ \(mol^{–1}\)
• B. 325 kJ \(mol^{–1}\)
• C. 399 kJ \(mol^{–1}\)
• D. 435 kJ \(mol^{–1}\)

Answer 1

The Correct Option is C

Wavelength of radiation = \(300\) \(nm\)

Photon energy

= \(\frac{hc}λ\)

= \(\frac{6.63 × 10^{-34} × 3 × 10^8}{300 × 10 ^{-19}}\)

= \(6.63 × 10^{-19}\) \(J\) 

Energy of \(1\) mole of photons

= \(6.63 × 10^{-19} × 6.02 × 10^{23} × 10^{-3}\)

= \(399\) \(kJ\)