Question

In: Chemistry

The bond disssociation of O2 is 498kJ/mol (i.e., it requires 498 kJ to take one mole...

The bond disssociation of O₂ is 498kJ/mol (i.e., it requires 498 kJ to take one mole of O₂ molecules and break the bonds to make two moles of O atoms). What wavelength photon, in nm, would posess the minimum energy to break one O₂ molecule into two O atoms?

Expert Solution

energy require to dissociate 1 mole of O₂ = 498 KJ = 498000 J

1 mole contain 6.022 10²³ molecule hence, to dissociate 6.022 10²³ molecule require energy = 498000 J

then to break 1 molecule of O₂ require energy = 1 498000 / 6.022 10²³ = 8.269678 10^-19 J

we know equation

E = hc / where,

E = energy of photon required = 8.269678 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) / (8.269678 10^-19)

= 2.4037212 10^-7 m

1m = 1 10⁹ nm

then 2.4037212 10^-7 m = 240.37 nm

240.37 nm wavelength of photon required to break one O₂ molecule in two O atom

queen_honey_blossom answered 1 year ago

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