A) \[8.18\times {{10}^{-31}}m\]
B) \[6.26\times {{10}^{-21}}m\]
C) \[4.91\times {{10}^{-7}}m\]
D) \[4.1\times {{10}^{-6}}m\]
Correct Answer: C
Solution :
Energy required to break one Cl-Cl bond \[=\frac{\text{Bond}\,\text{enegy}\,\text{permole}}{\text{Avogadro }\!\!'\!\!\text{ s}\,\text{number}}\] \[=\frac{243\times {{10}^{3}}}{6.02\times {{10}^{23}}}J\] Let the wavelength of the photon to cause rupture of one Cl-Cl bond be\[\lambda \], \[\lambda =\frac{hc}{E}=\frac{6.6\times {{10}^{8}}\times 6.02\times {{10}^{23}}}{243\times {{10}^{3}}}\] \[=\frac{119.196}{243}\times {{10}^{-34}}\times {{10}^{31}}\times {{10}^{-3}}\] Therefore, \[\lambda =4.91\times {{10}^{-7}}\,m.\] Hence, the correct option is [c].
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