To calculate the maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon, we will use the equation:
ΔE = hc/λ
Where:
ΔE is the energy required to break the bond, which is given as 839 kJ/mol.
h is the Planck constant (6.62607015 × 10^-34 J·s).
c is the speed of light (2.998 × 10^8 m/s).
λ is the wavelength of light.
First, let's convert the energy from kJ/mol to J:
ΔE = 839 kJ/mol * (1000 J/1 kJ) = 839,000 J/mol
To calculate the energy per photon, we need to divide ΔE by Avogadro's number (6.022 x 10^23 mol^-1):
Energy per photon = ΔE / Avogadro's number = 839,000 J/mol / (6.022 x 10^23 mol^-1) = 1.394 x 10^-18 J
Now we can rearrange the equation to solve for the wavelength:
λ = hc / ΔE
Substituting the known values:
λ = (6.62607015 × 10^-34 J·s * 2.998 × 10^8 m/s) / (1.394 x 10^-18 J)
λ = 143.31 nm
Therefore, the maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is approximately 143.31 nm (rounded to the correct number of significant digits).
It takes 839 kJ/mol to break a carbon carbon triple bond calculate the maximum wavelength of light for which a carbon carbon triple bond could be broken by absorbing a single photon
Be sure your answer has correct number of significant digits in nm
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1 answer