Answered: Calculate the energy of the violet…

Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm. O 1.23 x 10-19 J O 4.85 x 10-19 J O 5.27 x 10-19J O 2.06 x 10-19 J

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section20.3: Energy

Problem 3RC

See similar textbooks

Related questions

Q: Calculate the energy per photon of blue light of frequency 6.40 x 1014 Hz.

A: Given :- frequency of blue light = 6.40 × 1014 Hz To calculate :- Energy

Q: Calculate the kinetic energy of an electron moving at a speed of 3.88 x 105 m/s

A: Speed of an electron, ν = 3.88 × 105 m s-1 Mass of an electron, m = 9.11 × 10-31 kg Kinetic energy…

Q: Consider light with a wavelength of 1.25 x 10¬10 m. The energy of a single photon of this type of…

A: Photon will transfer its energy to the water molecules, and continuous bombardment of photon will…

Q: When a metal was exposed to photons at a frequency of 1.19 × 10'5 s-', electrons were emitted with a…

A: You can find the work function of the metal which is the energy required to free the electron from…

Q: A photon of light produced by a surgical laser has an energy of wavelength of 6.57 x 10-7 m.…

A: The energy of photon can be calculated by using formula

Q: Calculate the energy of 1.215 moles of light with a wavelength of 188.334 nm. 6.02 x 1023 things =…

A: Solution -

Q: In his explanation of the threshold frequency in the photoelectric field, Einstein reasoned that the…

A: Given that., Work function = 4.41 × 10-19 J And also work function = h × v v = frequency = c/λ λ =…

Q: Calculate the wavelength (in nm) of the red light emitted by a neon sign with a frequency of 4.74 x…

A: Given: frequency= 4.74 x 1014 Hz = 4.74 x 1014s-1 speed of light = 3 x 108 m/s

Q: A hydrogen lamp emits blue-green light with a wavelength of 486.1 nm. This corresponds to the…

A: Energy of photon is related to wavelength as, We…

Q: You are given the kinetic energy of ejected electrons as a function of wavelength for three…

A: It states that when a radiation of sufficient frequency strikes a metal surface, ejection of…

Q: the following energy levels of a hypothetical atom: 4:-1.21 × 10-¹9 J 3-7.41 × 10-19 J 2:-1.05 ×…

A: ΔE = En - Em ΔE is amount of energy absorbed or releasedWhere , m and n are no. of energy levels

Q: From the Lewis structures of the species given, pick all of those in which the central atom obeys…

A: As per the regulations only the first question can be answered.

Q: How many photons with a wavelength of 350 nm are needed to deliver a total of 7.52 x 10-14 joules of…

Q: What is the wavelength of light having a frequency of 4.27 x 104 Hz? O 585 O 702 O 641 O 522

A: Given data,Frequency(ν)=4.27×1014Hz The wavelength of a light is inversely proportional to the…

Q: Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm. 2.20…

Q: (a) A local radio station broadcasts at a frequency of 99.6 MHz (99.6 × 10° Hz). What is the…

A: Since you have posted a question with multiple subparts, we can answer only first three subparts. To…

Q: A photon shines on the surface of a piece of metal with the frequency of 1.37 x 1015 s1 Calculate…

A: Data given: Frequency of photon, f = 1.37×1015 s–1 Kinetic energy of emitted electron, KE =…

Q: Calculate the energy associated with the yellow line in the helium spectrum which has a wavelength…

Q: calculate the wavelength of light in nanometers that corresponds to a frequency of 7.25 x 10^14 Hz

A: Given: Frequency of light, v = 7.25 × 1014 Hz Formula used: Wavelength of light = speed of light…

Q: Calculate the energy of the red light emmitted by a neon atom with wavelength of 680 nm.

A: Energy(E) of light ray emitted from the source can be calculated by using Planck's law:

Q: Calculate the energy of a photon in the red light emitted by a neon sign with a wavelength of 703.2…

A: The energy of the radiation is quantized and the energy of one photon is given by: E = hv Where, h =…

Q: The electron in the hydrogen atom moves from the n = 3 to the n = 1 state. What is the energy of the…

Q: When the light of frequency 3.27 x 1015 s-1 shines on the surface of copper metal, electrons are…

Q: E4 = −1.0 × 10−19 J E3 = −5.0 ×10−19 J E2 = −1.0 × 10−18 J E1 = −1.5 ×…

A: Wavelength is related to energy by the following formula : E = h.Cλwhere λ = wave lengthE = energyh…

Q: When a red light with a wavelength of 670 nm shines on a piece of metal, an electron is ejected.…

A: Given -> Wavelength= 670 nm

Q: A wave has a wavelength of 32.87 μm, determine its frequency. 9.121 x 1012 5-1 O 1.096 x 10-13 S-1…

Q: Suppose an oven's radiation wavelength is 0.125 m. A container with 175.00 g of water was placed in…

Q: 104. Photogray lenses incorporate small amounts of silver chloride in the glass of the lens. The…

A: Given E = 3.10 x 102 kJ/mol = 3.10 x 105 J/mol

Q: Microwave ovens use microwave radiation to heat food. The energy of the microves is absorbed by…

A: 1.To calculate the energy of a photon with a wavelength of 11.2cm, use the Energy relation:

Q: A hydrogen lamp emits blue-green light with a wavelength of 486.1 nm. This corresponds to the…

A: 8.1x1018 will be correct option

Q: What is the energy (in joules) of a photon of green light having a wavelength of 440 nm?

Q: An atom emits light at various wavelengths, two of which are 434 nm and 472 nm. Both of these…

A: To determine the difference between the two state

Q: Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. 3.54 x…

Q: A photon of light with a wavelength of 200.0 nm strikes a metal surface and an electron is ejected…

Q: Which of the following forms of electromagnetic radiation have the longest wavelength? O Radio waves…

Q: A certain shade of blue has a frequency of 7.25×1014 Hz.7.25×1014 Hz. What is the energy ? of…

Concept explainers

Electronic Transitions and Spectroscopy

The term “electronic” connotes electron, and the term “transition” implies transformation. In a molecule, the electrons move from a lower to a higher energy state due to excitation. The two energy states, the ground state and the excited state are the lowest and the highest energy states, respectively. An energy change is observed with this transition, which depicts the various data related to the molecule.

Photoelectron Spectroscopy

Photoelectron spectroscopy (PES) is a part of experimental chemistry. It is a technique used in laboratories that involves projecting intense beams of radiation on a sample element. In response, the element ejects electrons for which the relative energies are measured.

Question

Calculate the energy of the violet light emitted by a hydrogen atom with a
wavelength of 410.1 nm.
O 1.23 x 10-19 J
4.85 x 10-19 J
O 5.27 x 10-19J
O 2.06 x 10-19 J
O 8.13 x 10-19 J

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Answer

Trending now

This is a popular solution!

Step by step

Solved in 5 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Ll.17.
Calculate the energy in kJ of 0.0130 moles of photon of light with wavelength of 640 nm. h = 6.626 x 10 34 J.s C = 3.00 x 108 m/s 2430 kJ 2.43 kJ 7.83 x 1021 kJ 3.11 x 1019 kJ O 1.56 kJ
A container with 0.2450.245 L of water is placed in a microwave and radiated with electromagnetic energy with a wavelength of 14.114.1 cm. The temperature of the water rose by 72.172.1 °C. Calculate the number of photons that were absorbed by the water. Assume water has a density of 1.00 g·mL−11.00 g·mL−1 and a specific heat of 4.184 J·g−1·°C−14.184 J·g−1·°C−1.
Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and molecules. High-energy radiation (usually UV or x-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the measured energy of the electron lost. The following energy differences were determined for several electron transitions: ΔΕ2–1 : 4.098 × 10-¹7 J AE5-1 = 5.242 × 10-¹7 J ΔΕ3-1 - = 4.854 × 10-17 J AE4-2= 1.024 × 10-¹7 J Calculate AE and λ of a photon emitted in the following transitions: (a) level 3 → 2; (b) level 4 → 1; (c) level 5 → 4.
What is the energy of a wavelength of light of 510 nm? O 1.01 x 10- 22 J O 3.90 x 10-37 J O 3.90 x 10-19J O 1.01 x 10-31 J
Find the frequency of a photon whose energy would be sufficient to cleave a Cl-Cl molecule. Use the Planck equation and the following data: - Planck’s constant = 6.63 x 10^-34 Js. The Avogadro Constant = 6.02 X 10^23 mol^-1 The Cl-Cl bond strength is 242 kJmol^-1
Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and mol ecules. High-energy radiation (usually UV or x-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the mea sured energy of the electron lost. The following energy differences were determined for several electron transitions: ∆E2→1 = 4.098x10-17 J ∆E3→£1 = 4.854x10-17 J ∆E5→1 = 5.242x10-17 J ∆E4→2 = 1.024x10-17 J Calculate ∆E and l of a photon emitted in the following transitions: (a) level 3 → 2; (b) level 4 → 1; (c) level 5→4.
What is the maximum wavelength capable of breaking an oxygen - oxygen bond in ozone? Both of the bonds in ozone are equivalent (1.5 bond order) and have a bond enthalpy of 362.8 kJ/mol. Group of answer choices 5.48 x 10-31nm 330 pm 330 nm 3.30 x 10-7 nm
Mg emits radiation at 285 nm. What is the frequency (Hz) of this radiation? O 1.05 x 10-3 O 1.05 x 101 O 1.05 x 1019 O 1.05 x 1015
How many photons are contained in a burst of yellow light (589. nm) from a sodium lamp that has 609. kJ of energy? 3.06 x 1030 photons 1.81 x 1024 photons 2.48 x 1025 photons 4.03 x 1028 photons 3.37 x 10¹⁹ photons
(3a-104-17) Would you agree to buy 1.23 x 1021 platinum atoms for $17? Explain why or why not, showing all work. The current price of platinum is 30.71 dollars/gram.
Electromagnetic radiation with a wavelength of 575 nm appears as yellow light to the human eye. If a laser emits 3.8 x 1016 photons of this energy in a pulse, what is the energy of the pulse in mJ?