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JEE Main & Advanced AIEEE Solved Paper-2010

  • question_answer
      The energy required to break one mole of \[ClCl\]bonds in\[C{{l}_{2}}\]is \[242\text{ }kJ\text{ }mo{{l}^{-1}}\]. The longest wavelength of light capable of breaking a single\[ClCl\]bond is (\[C=3\times {{10}^{8}}m{{s}^{-1}}\]and\[{{N}_{A}}\text{=}6.02\times {{10}_{23}}\text{ }mo{{l}^{-1}}\])       AIEEE  Solved  Paper-2010

    A) 494 nm

    B)                        594                        

    C)        640 nm

    D)        700 nm

    Correct Answer: A

    Solution :

    \[E=\frac{hc}{\lambda }\] \[=\frac{242\times {{10}^{+3}}}{6.02\times {{10}^{23}}}=\frac{6.62\times {{10}^{-34}}\times 3\times {{10}^{8}}}{\lambda }\] \[\lambda =\frac{6.62\times {{10}^{-26}}\times 3\times 6.02\times {{10}^{20}}}{242}\] \[=\frac{6.62\times 18.06\times {{10}^{-6}}}{242}\] \[=0.494\times {{10}^{-6}}=4.94\times 10{{\text{ }}^{-7}}m\] \[=494\text{ }nm\]


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