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aniked [119]
3 years ago
9

Problem Page Question It takes to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbo

n-carbon single bond could be broken by absorbing a single photon.
Chemistry
1 answer:
Marizza181 [45]3 years ago
5 0

This is a incomplete question. The complete question is:

It takes 348 kJ/mol to break a carbon-carbon single bond. Calculate the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon. Round your answer to correct number of significant digits

Answer: 344 nm

Explanation:

E=\frac{Nhc}{\lambda}

E= energy  = 348kJ= 348000 J  (1kJ=1000J)

N = avogadro's number = 6.023\times 10^{23}

h = Planck's constant = 6.626\times 10^{-34}Js


c = speed of light = 3\times 10^8ms^{-1}

348000=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}\times 3\times 10^8}{\lambda}

\lambda=\frac{6.023\times 10^{23}\times 6.626\times 10^{-34}\times 3\times 10^8}{348000}

\lambda=3.44\times 10^{-7}m=344nm    1nm=10^{-9}m

Thus the maximum wavelength of light for which a carbon-carbon single bond could be broken by absorbing a single photon is 344 nm

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To find for the oxidizing agent, first let us write the half reactions of this complete chemical reaction:

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Explanation:

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PH scale is used to determine how acidic , basic or neutral a solution is. It can be calculated using the following equation 
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A chemistry student is performing a lab exercise where they are reacting aqueous Lead (II) Nitrate with aqueous Potassium Iodide
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