In: Chemistry
Please show all work.
3. The dissociation of the HO-H bond in water requires 493 kJ/mol.
a) How much energy, in joules, is required to break the HO-H bond in a single water molecule?
b) What wavelength of electromagnetic radiation would have the energy required to break a HO-H bond?
c) In what region of the spectrum (X-ray, UV, Vis, IR, etc.) does this radiation appear?
a) 493 KJ = 493000 J
Thus, the dissociation of the HO-H bond in water requires 493000 J/mol
According to avogadro's law 1 mole of water contain 6.022
1023
molecule that mean 6.022
1023
molecule require 493000 J energy then 1 molecule of water require
493000 / 6.022
1023
= 8.186649
10-19
J of energy
to break the HO-H bond in a single water molecule require
8.186649 10-19
J of energy
b)
E = hc / where,
E = energy = 8.186649 10-19
J
h = Planck constant = 6.62610-34J
s
c = velocity of light = 3.00108
m/s
= wavelength in
meter
we can wright above equation
= hc/E
Substitute value
=
(6.626
10-34)
(3.00
108) /
(8.186649
10-19)
= 2.428
10-7
meter = 242.8 nm
242.8 nm wavelength of electromagnetic radiation would have the energy required to break a HO-H bond
c) It is come in UV region
because UV region have range between 100 nm to 400 nm