To calculate the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon, we need to use the equation:
E = hc/λ
where E is the energy required to break the bond (498 kJ/mol), h is Planck's constant (6.62607015 x 10^-34 J·s), c is the speed of light (2.998 x 10^8 m/s), and λ is the wavelength of light.
First, let's convert the energy required to joules (J) from kJ/mole to J/mole:
498 kJ/mol = (498 x 10^3) J/mol = 4.98 x 10^5 J/mol
Now, we can rearrange the equation to solve for λ:
λ = hc/E
λ = (6.62607015 x 10^-34 J·s)(2.998 x 10^8 m/s)/(4.98 x 10^5 J/mol)
λ = (1.98644582 x 10^-25 J·m)/(4.98 x 10^5 J/mol)
λ = 3.98839259 x 10^-31 m/mol
Finally, we can convert m/mol to nm:
(3.98839259 x 10^-31 m/mol)(10^9 nm/1 m) = 3.98839259 x 10^-22 nm/mol
Therefore, the maximum wavelength of light for which an oxygen-oxygen double bond could be broken by absorbing a single photon is approximately 3.99 x 10^-22 nm, using the correct number of significant digits.
It takes 498kJ/mol to break a oxygen oxygen doublebond calculate the maximum wavelength of light for which a oxygen oxygen double bond could be broken by absorbing a single photon
Be sure your answer has correct number of significant digits in nm
1 answer