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Standard XII

Chemistry

1900's Physics and Wave

O 2 undergoes...

Question

$O_{2}$ undergoes photochemical dissociation into one normal oxygen atom and one oxygen atom which is 1.5 $e V$ more energetic than normal. The dissociation of $O_{2}$ into two normal atoms of oxygen requires 504 $k J m o l^{- 1}$ . What is the maximum wavelength effective for photochemical dissociation of $O_{2}$ ?

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Solution

$O_{2} h v \to O_{N o r m a l} + O_{E x c i t e d}$
$O_{2} \to O_{N o r m a l} + O_{N o r m a l}$
Energy rquired for simple dissociation of $O_{2}$ into two normal atoms = $\frac{504 \times 10^{3}}{6 \times 10^{23}} J$
If one atom in excited state has more energy, i.e, 1.5 $e V$
= $1.5 \times 1.6 \times 10^{- 19} J$
So, the energy required for photochemical dissociation of $O_{2}$ is,
= $\frac{504 \times 10^{3}}{6 \times 10^{23}}$ + $1.5 \times 1.6 \times 10^{- 19} = 10.8 \times 10^{- 19} J$
$E = \frac{h c}{λ}$
$10.8 \times 10^{- 19} = \frac{6 \times 10^{- 34} \times 3 \times 10^{8}}{λ}$

$λ = 1666.67 0 A$

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O2 undergoes photochemical dissociation into one normal oxygen atom and one oxygen atom which is 1.5 eV more energetic than normal. The dissociation of O2 into two normal atoms of oxygen requires 504 kJmol−1. What is the maximum wavelength effective for photochemical dissociation of O2?