Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. The Cl – Cl bond energy is 243 kJ m o l - 1 ( h = 6.6 × 1 0 - 34 J s ; c = 3 × 1 0 8 m / s ; Avogadro’s number = 6.02 × 1 0 23 m o l - 1 )

Question

Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. The Cl – Cl bond energy is 243 kJ m o l - 1 ( h = 6.6 × 1 0 - 34 J s ; c = 3 × 1 0 8 m / s ; Avogadro’s number = 6.02 × 1 0 23 m o l - 1 ), 8.18 × 1 0 - 31 m, 6.26 × 1 0 - 21 m, 4.905 × 1 0 - 7 m, 4.1 × 1 0 - 6 m

MARKS App · Accepted Answer

Energy required to break one Cl − Cl bond = b o n d e n e r g y p e r m o l e A v o g a d r o ’ s n u m b e r = 243 × 1 0 3 6.02 × 1 0 23 J Let the wavelength of the photon to cause rupture of one Cl – Cl bond be λ, λ = h c E = 6.6 × 1 0 - 34 × 3 × 1 0 8 × 6.02 × 1 0 23 243 × 1 0 3 = 119.196 243 × 1 0 - 34 × 1 0 31 × 1 0 - 3 = 4.905 × 1 0 - 7 m .

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