Answer:
The wavelength of light require to brake an single I-I bond is 7.92 × 10⁻⁷ m
Explanation:
Amount of energy required to break the one mole of iodine-iodine single bond = 151 KJ
amount of energy to break one iodine -iodine bond = (151 KJ/mol )/ 6.02 × 10²³/mol = 2.51 × 10⁻²² KJ
or
2.51 × 10⁻¹⁹ J
Formula:
E = hc / λ
h = planck's constant = 6.626 × 10⁻³⁴ js
c = speed of light = 3 × 10⁸ m/s
λ = wavelength
Solution:
E = hc / λ
λ = hc / E
λ = (6.626 × 10⁻³⁴ js × 3 × 10⁸ m/s ) / 2.51 × 10⁻¹⁹ J
λ = 19.878 × 10⁻²⁶ j .m / 2.51 × 10⁻¹⁹ J
λ = 7.92 × 10⁻⁷ m
The maximum wavelength of light for which an iodine-iodine single bond can be broken is [tex]7.92 \times 10^-^7 m[/tex]
Bonds are those which join atoms and molecules together. There are different types of bonds to different molecules.
The energy required to break one mole of iodine-iodine single bond, 151 kJ/mol.
The energy to break one iodine -iodine bond is
[tex]\dfrac{(151 KJ/mol )}{ 6.02 \times 10^2^3/mol } = 2.51 \times 10^-^2^2 KJ[/tex]
Now, from the plank's equation
E = hc / λ
h = planck's constant is [tex]6.626 \times 10^-^3^4 \;Js[/tex]
c = speed of light is [tex]3 \times 10^8 m/s[/tex]
λ = wavelength
[tex]E = \dfrac{hc}{\lambda } \\\\\lambda = \dfrac{hc}{E} \\\\\\\lambda = \dfrac{(6.626 \times 10^-^3^4 js \times 3 \times 10^8 m/s ) }{2.51 \times 10^-^1^9 J} \\\\\lambda =\dfrac{19.878 \times 10^-^2^6 j .m}{2.51 \times 10^-^1^9 J} = 7.92 \times 10^-^7m[/tex]
Thus, The maximum wavelength of light for which an iodine-iodine single bond can be broken is [tex]7.92 \times 10^-^7 m[/tex]
Learn more about bonds, here:
https://brainly.com/question/13559242
