Atomic chlorine is produced under ozone-hole conditions by the photodissociation of Cl2. Given that Cl2 gas...

Atomic chlorine is produced under ozone-hole conditions by the photodissociation of Cl2. Given that Cl2 gas is the most stable form of the element, and that the ΔHfo for atomic chlorine is +121.7 kJ mol-1, calculate the maximum wavelength of light that can dissociate diatomic chlorine into the monoatomic form. Does this wavelength correspond to the UVA or UVB region of the wavelength spectrum?

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Expert Solution

ΔHfo for atomic chlorine is +121.7 kJ mol-1

so that , DH0 dissociation of Cl2 = 121.7*2 = +243.4 Kj/mol

1 Cl2 molecule required energy = 243.4*10^3/(6.023*10^23) = 4.04*10^-19 joule

suitable wavelength (l) = hc/E = (6.625*10^-34*3*10^8)/(4.04*10^-19)

= 4.92*10^-7 m

= 492 nm

suitable light = visible region.

queen_honey_blossom answered 1 year ago

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