Calculate the wavelength of the light required to break the bond between two chlorine atoms in a chlorine molecule. The Cl - Cl bond energy is 243 kJ mol^(-1) (h = 6.6 xx 10^(-34) Js, c = 3 xx 10^(8) ms^(-1), Avogadro's number = 6.02 xx 10^(23) mol^(-1))

Calculate the wavelength of the light required to break the bond betwe

1.	Calculate the wavelength of the light required to break the bond between two chlorine atoms in a chlorine molecule. The Cl - Cl bond energy is 243 kJ mol^(-1) (h = 6.6 xx 10^(-34) Js, c = 3 xx 10^(8) ms^(-1), Avogadro's number = 6.02 xx 10^(23) mol^(-1))
Answer» `8.18 xx 10^(-31) m` `6.26 xx 10^(-21) m` `4.91 xx 10^(-7)m` `4.11 xx 10^(-6) m` Solution :Energy required to break one `Cl - Cl` bond `= ("Bond energy per mole")/("Avogado's No.") = (243 xx 10^(3) J)/(6.02 xx 10^(23))` `= 40.36 xx 10^(-20)J` `E =HV = h (c)/(LAMDA)` `:. lamda = (hc)/(E) = ((6.6 xx 10^(-34) Js) (3 xx 10^(8) ms^(-1)))/(40.36 xx 10^(-20) J)` `= 4.91 xx 10^(-7) m`