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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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Answer:

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2 years ago
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or,
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                            Mass       =  Moles × M.mass
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