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MariettaO [177]
3 years ago
8

X rays have wavelengths on the order of 1 3 10210 m. calcu‑ late the energy of 1.0 3 10210 m x rays in units of kilojoules per m

ole of x rays. (1 mol x rays 5 6.022 3 1023 x rays.) am radio waves have wavelengths on the order of 1 3 104 m. cal‑ culate the energy of 1.0 3 104 m radio waves in units of kilo‑ joules per mole of radio waves. consider that the bond energy of a carbon–carbon single bond found in organic compounds is 347 kj/mol. would x rays and/or radio waves be able to disrupt organic compounds by breaking carbon–carbon single bonds?
Physics
1 answer:
kondor19780726 [428]3 years ago
5 0

Answers:

a) E_{Xrays}=1.19(10)^{6} kJ/mol

b) E_{AM}= 1.19(10)^{-8} kJ/mol

c) X rays have the energy to disrupt organic compounds by breaking carbon–carbon single bonds, but AM radio waves not.

Explanation:

The energy of a photon in Joules is given by the following formula:

E=\frac{hc}{\lambda} (1)

However, if we want to know this energy in units of J/mol, we have to use the following formula:

E=\frac{hc}{\lambda} NA (2)

<h2>a) Now, in the case of X rays:</h2>

E_{Xrays}=\frac{hc}{\lambda_{Xrays}} NA (3)

Where:

E_{Xrays} is the energy of X rays in Joules (J)

h=6.6260701509 (10)^{-34} J.s is the Planck constant

c=3(10)^{8}m/s is the speed of light

\lambda_{Xrays}=1(10)^{-10}m is the wavelength of X rays

NA=6.0221(10)^{23}/mol is the Avogadro's number

E_{Xrays}=\frac{(6.6260701509 (10)^{-34} J.s)(3(10)^{8}m/s)}{1(10)^{-10}m}(6.0221(10)^{23}/mol) (4)

E_{Xrays}=1.19(10)^{9}J/mol=1.19(10)^{6} kJ/mol (5) This is the energy of X rays in units of kilojoules per mole

<h2>b) For AM radio waves:</h2>

E_{AM}=\frac{hc}{\lambda_{AM}} NA (6)

Where:

E_{AM} is the energy of AM radio waves in Joules (J)

\lambda_{AM}=1(10)^{4}m is the wavelength of AM wavelength

E_{AM}=\frac{(6.6260701509 (10)^{-34} J.s)(3(10)^{8}m/s)}{1(10)^{4}m} 6.0221(10)^{23}/mol (7)

E_{AM}=1.19(10)^{-5} J/mol= 1.19(10)^{-8} kJ/mol (8) This is the energy of AM radio waves in units of kilojoules per mole

<h2>c) Which is able to disrupt carbon–carbon single bonds?</h2>

If we compare the energy of both (X rays and AM radio waves) with the energy of a carbon–carbon single bond (347 kJ/mol), we will have the following:

1.19(10)^{6} kJ/mol > 1.19(10)^{-8} kJ/mol > 347 kJ/mol

This means the energy of X rays is greater than the energy of AM radio waves and greater than the energy of carbon–carbon single bond as well:

E_{Xrays} > E_{AM} > E_{carbon}

In addition, this means X rays have the energy to disrupt organic compounds by breaking carbon–carbon single bonds, but AM radio waves not.

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