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Determine the energy of 1.10 mol of photons for each of the following kinds of light.

infrared radiation (1580 nm )

visible light (520 nm )

ultraviolet radiation (170 nm )

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The energy of the photons are;

infrared radiation - 8.3* 10^4 J  

visible light - 2.52 * 10^5 J

ultraviolet radiation - 7.72 * 10^5 J

How do we find the energy?

The energy of photon could be found by the use of the of the equation;

E = hc/λ * 6.023 * 10^23/1 mole

E = energy of the photon

c = speed of light

λ = wavelength of the photon

Now;

For infrared radiation;

E = 6.6 * 10^-34 * 3 * 10^8/1580 * 10^-9 * 6.023 * 10^23/1 mole * 1.10 mol

E = 8.3* 10^4 J  

For visible light;

E = 6.6 * 10^-34 * 3 * 10^8/520 * 10^-9 * 6.023 * 10^23/1 mole * 1.10 mol

E = 2.52 * 10^5 J

For ultraviolet radiation;

E = 6.6 * 10^-34 * 3 * 10^8/170 * 10^-9 * 6.023 * 10^23/1 mole * 1.10 mol

E= 7.72 * 10^5 J

Learn more about photons:https://brainly.com/question/20912241

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