Answer:
3.53*10^{-7} m
Explanation:
Photon that can rupture the bonds are those with the energy of the bond dissociation energy. If we want to know the energy for each molecule we have to take into account that:
[tex]1mol=6.022*10^{23}molecule[/tex]
Hence, we have
[tex]E_d=339\frac{10^{3}J}{mol}*\frac{1mol}{6-022*10^{23}molecules}=5.62*10^{-19}J/molecule[/tex]
but the energy is also:
[tex]E_d=h\nu =\frac{hc}{\lambda}\\\\\lambda=\frac{hc}{E_d}[/tex]
where h is the Planck's constant and c is the speed of ligth. By replacing we obtain:
[tex]\lambda=\frac{(6.62*10^{-34}Js)(3*10^{8}m/s)}{5.62*10^{-19}J}=3.53*10^{-7}m[/tex]
hope this helps!
Answer:
3.53*10^-7 color white "m
Where h= Planck constant
C=speed of light
Explanation:
Calculating energy required to dissociate the cl--cl Bond as this
Energy= +339*color white*kJmol
E=(339*10^3/6.022*10^23)=5.63*10^-19color white
But note from Planck equation
E=hf=h*c/lamda
Lamda= hc/E
=6.63*10^-34*3*10^8/5.63*10^-19
Lamda=3.532*10^-7 colorwhite*m
