JEE CHEMISTRY MCQ: STRUCTURE OF ATOM

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Application +4 | -1

Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. The

\mathrm{Cl}-\mathrm{Cl}

bond energy is

243 \mathrm{KJ} / \mathrm{mol} .\left(h=6.6 \times 10^{-34} \mathrm{Js}\right)

View answer and explanation

Correct option: A

4.91 \times 10^{-7} \mathrm{m}

Option A (

4.91 \times 10^{-7} \mathrm{m}

) is correct because the wavelength is calculated using the energy required to break the Cl-Cl bond and the Planck's equation.

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\mathrm{A}

\times 10^{12}

\frac{1}{{ }^{\prime} \mathrm{B}^{\prime}}

\ell = 1,\,\,m = 0

1.25 \times {10^{ - 13}} \times {A^{1/3}}\mathrm{cm}.