Part 1 (1 point) What is the energy of a photon of UV light with a wavelength of 2.01×10^-7 m? The speed of light is c = 3.00 × 10^8 m/s, and Planck's constant is h = 6.626 × 10^-34 J · s. Part 2 (1 point) UV radiation interacts with matter in various ways and is capable of breaking covalent bonds. Which range of wavelengths represents UV radiation that can break a C–C bond with a bond energy of 345 kJ/mol? Assume that 1 mole of photons is absorbed for every 1 mole of bonds broken. Choose one: A. 372 nm to 385 nm B. 390 nm to 400 nm C. 331 nm to 347 nm D. 352 nm to 364 nm
Added by Teresa M.
Close
Step 1
626 \times 10^{-34} \, J \cdot s\) \(c = 3.00 \times 10^8 \, m/s\) \(\lambda = 2.01 \times 10^{-7} \, m\) ** Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 57 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
What is the frequency of UV radiation having a wavelength of 158.1 nm? a. 170.5 Hz b. 1.898*10^6 Hz c. 1.898*10^15 Hz d. 5.271*10^-9 Hz e. 5.271*10^14 Hz 2. Remote control units for electronic devices often operate in the IR region and require a "line of sight" to be effective, what is the wavelength if the frequency is 3.185*10^14 Hz? a. 1.06*10^6 m b. 9.42 nm c. 94.2 nm d. 942 nm e. 1.06*10^9 m 3. What is the energy, in Joules, of one photon of visible light with a wavelength of 464.1 nm? a. 1.026*10^-48 J b. 2.100*10^35 J c. 2.341*10^11 J d. 4.283*10^-19 J e. 6.372*10^-17 J 4. Which of the following is true regarding electromagnetic radiation? a. Energy is directly proportional to wavelength. b. Wavelength is directly proportional to frequency. c. Frequency is directly proportional to energy. d. A photon is a non-quantized particle of radiation. 5. Which of the following photons would have the highest energy a. 10.28 m b. 5.28 cm c. 5.17*10^-4 m d. 1.08*10^-6 m e. 3.14 nm 6. Which of the following is your favorite color? a. Red (650 nm) b. Orange (600 nm) c. Yellow (580 nm) d. Green (540 nm) e. Blue (440 nm)
Madhur L.
Which of the following photons has the highest energy? E = (hc)/λ, where c = 2.998x 10^8 m/sec; h = 6.626x 10^-34 J sec Photon with λ = 1.064 um, photon with v = 5.83x 10^14 Hz Photon with λ = 647 nm, photon with v = 1.55x 10^15 Hz Photon with λ = 633 nm What wavelength of light is required to cause the ejection of photoelectrons with kinetic energies of 5.0x 10^-20 J from a calcium surface (Φ = 4.60x 10^-19 J)? E = hv - KEelectron c = λv c = 2.998x 10^8 m/sec; h = 6.626x 10^-34 J sec 485 nm 390 nm 308 nm 632 nm 480 nm What is the energy (E, in joules) of the 514.5 nm photons emitted by an argon-ion laser? E = (hc)/λ, where c = 2.998x 10^8 m/sec; h = 6.626x 10^-34 J sec 4.29x 10^-36 J 2.33x 10^35 J 4.29x 10^-45 J 3.86x 10^-19 J 3.86x 10^-28 J
Adi S.
1. The energy for one state of the H atom is -2.42 × 10 -19 J. What frequency (Hz) of light would need to be emitted to reach a state with an energy of -2.18 × 10 -18 J? Express answer in scientific notation. 2. A H atom emitts a photon with a wavelength of 1.22 × 102 nm. If the energy of the initial state of the H atom was -5.45 × 10(-19) J, calculate the energy of the final state. Express answer in scientific notation. 3. A Li2+ ion emitts a photon with a frequency of 2.22 × 1016 Hz. If the energy of the initial state of the Li2+ ion was -4.91 × 10(-18) J, calculate the energy of the final state. Express answer in scientific notation.
Umar Sohail Q.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD