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One requires $11 \mathrm{eV}$ of energy to dissociate a carbon monoxide molecule into carbon and oxygen atoms. The minimum frequency of the appropriate electromagnetic radiation to achieve the dissociation lies in
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Verified Answer
The correct answer is:
ultraviolet region
ultraviolet region
As we know that,
$$
E=h v
$$
As given that $\mathrm{h}=6.62 \times 10^{-34} \mathrm{~J}-\mathrm{s}$
$\mathrm{E}=11 \mathrm{eV}=11 \times 1.6 \times 10^{-19}$
$v=$ ?
$11 \mathrm{eV}=\mathrm{hv}$
So, $v=\frac{11 \times 1.6 \times 10^{-19}}{\mathrm{~h}} \mathrm{~J}=\frac{11 \times 1.6 \times 10^{-19}}{6.62 \times 10^{-34}} \mathrm{~J}$ $=2.65 \times 10^{15} \mathrm{~Hz}$
So, that frequency radiation belongs to ultraviolet region.
$$
E=h v
$$
As given that $\mathrm{h}=6.62 \times 10^{-34} \mathrm{~J}-\mathrm{s}$
$\mathrm{E}=11 \mathrm{eV}=11 \times 1.6 \times 10^{-19}$
$v=$ ?
$11 \mathrm{eV}=\mathrm{hv}$
So, $v=\frac{11 \times 1.6 \times 10^{-19}}{\mathrm{~h}} \mathrm{~J}=\frac{11 \times 1.6 \times 10^{-19}}{6.62 \times 10^{-34}} \mathrm{~J}$ $=2.65 \times 10^{15} \mathrm{~Hz}$
So, that frequency radiation belongs to ultraviolet region.
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