Question

hey guys Good Morning ....
plz help me out ....answer the above question ......​

Answer 1

$\huge\underline{\underline{\bf \green{Solution-}}}$

$\large{\sf Cl_2\:\:\:→\:\:\:2Cl}$ ∆H = +242 kJ/mol

Energy required to break one molecule of ${\sf Cl_2}$

$\implies{\sf E = \dfrac{242×10^3}{6.023×10^{23}}}$

$\implies{\bf \blue{E = 4.01×10^{-19}J}}$

✪$\large{\boxed{\bf \blue{\lambda =\dfrac{hc}{E}} }}$

$\implies{\sf \dfrac{6.63×10^{-34}×3×10^8}{4.01×10^{-19}} }$

$\implies{\sf \dfrac{19.89×10^{-26}}{4.01×10^{-19}}}$

$\implies{\sf 4.94×10^{-7} }$

$\implies{\bf \red{\lambda = 494\:nm} }$

$\huge\underline{\underline{\bf \green{Answer-}}}$

Option (b) 494 nm

Longest Wavelength of the light capable of breaking single Cl⎯Cl bond is ${\bf \red{494\:nm}}$

Answer 2

(b) 494nm...... is ur answer