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swat32
3 years ago
5

The carbon-carbon (C―C) bond has an average bond energy of 347 kJ/mol, which is the energy required to break one mole of C―C bon

ds. What is the wavelength of the photon that can break this bond? 487 nm 457 nm 354 nm 345 nm 377 nm
(1) 457 nm
(2) 487 nm
(3) 345 nm
(4) 354 nm
(5) 377 nm
Chemistry
1 answer:
olganol [36]3 years ago
6 0

Answer:

(3) 345 nm

Explanation:

<u>Given:</u>

Average C-C bond energy = 347 kJ/mol

<u>To determine:</u>

Wavelength of photon that can break a C-C bond

<u>Calculation:</u>

The energy (E) of a photon is related to its wavelength (λ) by the Planck's equation:

E = \frac{hc}{\lambda }

where h = Planck's constant = 6.626*10⁻³⁴ Js

c = speed of light = 3*10⁸ m/s

\lambda = \frac{hc}{E}

\lambda =\frac{6.626*10^{-34}Js*3*10^{8}ms^{-1}*6.023*10^{23}mol^{-1}}{347,000Jmol^{-1}}

λ = 3.45*10⁻⁷ m

Since 1 nanometer (nm) = 10⁻⁹ m

The calculated wavelength corresponds to 345 nm

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<h3>What is ozonolysis?</h3>

Ozonolysis is a reaction used in organic chemistry to determine the position of a carbon-carbon double bond in unsaturated compounds.

i. The given alkene X, that is subject to ozonolysis would be 2-methyl-2-pentene. Upon exposure to ozone, an ozonide is initially formed, after which it is broken down into 2 products - acetone and propanal, both with the molecular formula C₃H₆O.

The given compound X is 2-methyl pent-2-ene. When it is reacted with ozone it forms an ozonide in the first step. In the second step the reduce to forms acetone and propanal.

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