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qwelly [4]
2 years ago
13

Radiation in the ultraviolet region of the electromagnetic spectrum is quite energetic. It is this radiation that causes dyes to

fade and your skin to develop a sunburn. If you are bombarded with 1. 00 mol of photons with a wavelength of 370. Nm, what amount of energy, in kilojoules per mole of photons, are you being subjected to? energy mol submit answer try another versiorn 2 item attempts remaining.
Physics
1 answer:
N76 [4]2 years ago
5 0

The  energy of photon in kJ/mol is 329kJ/mol.

Wavelength of radiation is 370nm. The frequency of given wavelength is

            ν = c / λ

            ν = 3×10^8 / 370×10^-9

            ν = 8.11 × 10^14 s^-1

      Now the energy of photon is:

             E = hν

             E = 6.63×10^-34  J.s/photon × 8.11×10^14s^-1

             E = 5.41× 10^-19  J/photon

         To find in mole

              E = 5.41× 10^-19 × 6.022×10^23

               E = 3.29 ×10^ 5 J/mol

   So, the energy of mole of photon is equal to 329 kJ/mol.

        Learn more about radiation here:

                brainly.com/question/18650102

                     #SPJ4  

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Answer:

a) a=33.73mm/s^{2}

b) mg>N

c) \%_{change}=0.343\%

d) a=24.07mm/s^{2}

Explanation:

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a_{c}=33.73mm/s^{2}

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N=mg-ma_{c}

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mg>mg-ma_{c}

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N=m(g-a_{c})

N=(60kg)(9.81m/s^{2}-33.73x10^{-3}m/s^{2})

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\%_{change} = \frac{588.6N-586.58N}{588.6N} x 100\%

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a=(72.72x10^{-6} rad/s)^{2}(4,551.91x10^{3}m

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