Question

In: Chemistry

Please show all work. 3. The dissociation of the HO-H bond in water requires 493 kJ/mol....

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?

Expert Solution

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

= (6.62610^-34)(3.0010⁸) / (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

queen_honey_blossom answered 1 year ago

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