Question

Be sure to answer all parts. Without stratospheric ozone (O3), harmful solar radiation would cause gene alterations. Ozone forms when the bond in O2 breaks and each O atom reacts with another O2 molecule. It is destroyed by reaction with Cl atoms formed when the C―Cl bond in synthetic chemicals breaks. Find the wavelengths of light that can break the C―Cl bond and the bond in O2. Give your answers in scientific notation. C―Cl × 10 m O2 × 10 m

Answer 1

Answer:

for C-Cl  bond $\lambda_1=3.66\times 10^{-9}\ m$

for O-O bond $\lambda_2=2.43\times 10^{-9}\ m$

Explanation:

• We have the bond enegy for C-Cl, $BE_1=327\ kJ.mol^{-1}= 327000\times 1.66\times 10^{-22}\ J\ per\ molecule$

• bond enegy for C-Cl, $BE_2=494\ kJ.mol^{-1}= 494000\times 1.66\times 10^{-22}\ J\ per\ molecule$

Now as we know the energy of electromagnetic waves is given by:

$E=h.\nu$

here E = BE

Then for C-Cl:

$327000\times 1.66\times 10^{-22}=6.63\times 10^{-34}\times \nu_1$

$\nu_1=8.18733\times 10^{16}\ Hz$

Now wavelength:

$\lambda_1=\frac{c}{\nu_1}$

$\lambda_1=\frac{3\times 10^8}{8.18733\times 10^{16}}$

$\lambda_1=3.66\times 10^{-9}\ m$

For O2:

$494000\times 1.66\times 10^{-22}=6.63\times 10^{-34}\times \nu_2$

$\nu_2=1.236863\times 10^{17}\ Hz$

Now wavelength:

$\lambda_2=\frac{c}{\nu_2}$

$\lambda_2=\frac{3\times 10^8}{1.236863\times 10^{17}}$

$\lambda_2=2.43\times 10^{-9}\ m$