Respuesta :
Answer :
(1) The frequency of photon is, [tex]3\times 10^{10}Hz[/tex]
(2) The energy of a single photon of this radiation is [tex]1.988\times 10^{-23}J/photon[/tex]
(3) The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol
Explanation : Given,
Wavelength of photon = [tex]1.0cm=0.01m[/tex] (1 m = 100 cm)
(1) Now we have to calculate the frequency of photon.
Formula used :
[tex]\nu=\frac{c}{\lambda}[/tex]
where,
[tex]\nu[/tex] = frequency of photon
[tex]\lambda[/tex] = wavelength of photon
c = speed of light = [tex]3\times 10^8m/s[/tex]
Now put all the given values in the above formula, we get:
[tex]\nu=\frac{3\times 10^8m/s}{0.01m}[/tex]
[tex]\nu=3\times 10^{10}s^{-1}=3\times 10^{10}Hz[/tex] [tex](1Hz=1s^{-1})[/tex]
The frequency of photon is, [tex]3\times 10^{10}Hz[/tex]
(2) Now we have to calculate the energy of photon.
Formula used :
[tex]E=h\times \nu[/tex]
where,
[tex]\nu[/tex] = frequency of photon
h = Planck's constant = [tex]6.626\times 10^{-34}Js[/tex]
Now put all the given values in the above formula, we get:
[tex]E=(6.626\times 10^{-34}Js)\times (3\times 10^{10}s^{-1})[/tex]
[tex]E=1.988\times 10^{-23}J/photon[/tex]
The energy of a single photon of this radiation is [tex]1.988\times 10^{-23}J/photon[/tex]
(3) Now we have to calculate the energy in J/mol.
[tex]E=1.988\times 10^{-23}J/photon[/tex]
[tex]E=(1.988\times 10^{-23}J/photon)\times (6.022\times 10^{23}photon/mol)[/tex]
[tex]E=11.97J/mol[/tex]
The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol
Answer:
Do you do professor Huang's Chemistry Class?
Explanation:
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