The rays of the Sun that cause tanning and burning are in the ultraviolet portion of the electromagnetic spectrum. These rays are categorized by wavelength: So-called UV-A radiation has wavelengths in the range of 320-380 nm, whereas UV-B radiation has wavelengths in the range of 290-320 nm. Part B Calculate the energy of a mole of 330 nm photons. 17 ΑΣΦ E= 10 Submit 45 f T Previous Answers Request Answer ? X Incorrect; Try Again; 2 attempts remaining kJ/mol

Given: =AV NA-6.022 x10 23 E=hv 1 nm 1x10 m E= hc/N ITH2 = 1 x10-4 Hz 12 c-2.998 x10° m/s |I MHz = 1x10° Hz h=6,626x104 What is the energy of one mole of photons with a 0.552 m wavelength? Include units and correct significant figures as part of your answer.

Determine the energy of 1.20 mol of photons for each of the following kinds of light.

German physicist Werner Heisenberg related the uncertainty of an object's position (Ax) to the uncertainty in its velocity (Av) h Ax 2 4xmAv where h is Planck's constant and m is the mass of the object. The mass of an electron is 9.11 x 10-31 kg. What is the uncertainty in the position of an electron moving at 5.00 x 10° m/s with an uncertainty of Av = 0.01 x 10ʻ m/s? Ax 2 m

Now try and rearrange the E = hc/Aequation so that you can find the wavelength of a photon that has an energy of 5.15 x 10-19 J. Type your answer here nm You are incorrect Hint When you do a wavelength calculation your wavelength must have units of meters to match the units of the speed of light! Answered - Incorrect Fullscreen 1 Resubmit %23 12:00 AM の 昂 4/30/2021 prt sc delete home end pg up 10 num backspace 8. lock 8. 6. Y home pg up 4. 6. enter G H. K pause ↑ shift pg end alt ctrl ins

Calculate the frequency of light (in s1 also known as Hz) with a wavelength of (6.00x10^2) nm. Use a value of (3.0000x10^8) for the speed of light. Remember 1 m%3D (1.0000x10^9) nm Do not include units with your answer. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10 Answer

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Calculate the energy (in J) of a mol of photons with a wavelength of 450.0 nm (a shade of blue light). Upload a picture of your answer, showing all work. Given:   E=hυ υ : frequency, in s-1 (Hertz, Hz) E= hc/λ λ is wavelength, in m c=λυ h=6.626 x10-34 Js (Planck’s constant) E: energy of a photon (in J) c=2.998 x108 m/s (speed of light) 1 nm = 1x10-9 m

What is the wavelength in nm of a photon emitted from an H atom if an electron transfers from n=6 to n=3     RH = Rydberg constant = 1.097 x 10 -2  nm-1 Your answer should have 4 sig figs.

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