Calculate the energy (in joules) of a photon with a wavelength of 5.00 × 103 nmPlanck's constant is 6.626 X 10-34 J.s.: c = %v; E=hv; speed of light =c = 3.00 X 10° m/s;v = frequency; =wavelengthfiauration for iodine.

Answer Energy of a photon = 3.9756*10-20 J

Answered: Calculate the energy (in joules) of a…

Science

Chemistry

Calculate the energy (in joules) of a photon with a wavelength of 5.00 × 10° nm

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

Problem 5.ACP

See similar textbooks

Related questions

Q: What is the energy (in J) of a photon of light with a frequency of 5.0 x 10^15 Hz?

A: Energy of an electromagnetic radiation is governed by frequency or wavelength of associated…

Q: What is the energy of a mole of photons that have a wavelength of 723 nm? (h = 6.626 × 10⁻³⁴ J • s…

A: We know that , energy of a photon is related to Plank's constant as,…

Q: Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of…

A: Given data Frequency of mercury lamp = 5.49 × 1014 Hz We have to calculate the energy of the green…

Q: What is the minimum number of microwave photons with a wavelength of 3.36 mm that will have to be…

A: Calculation of heat required to heat the water:

Q: I calculated the energy of 1 mole of photons with a wavelength lambda of 625 nm to be 3.18 x 10-19…

A: In the study of physics and chemistry, understanding the relationship between the energy of photons…

Q: Determine the energy of a photon with a wavelength of 319 nm ( h=6.626x10^-34j•s and c=3.00x10^8…

Q: What is the wavelength (in pm) of a proton traveling at a speed of 6.21 km/s?

A: The wavelength (in pm) of a proton travelling at a speed of 6.21 km/s is calculated as,

Q: Calculate the wavelength (in meters) of a photon emitted by a carbon atom when its electron drops…

Q: What is the frequency (in Hertz) of a photon with an energy value of 6.03 x 10-18?

Q: Thermal neutrons are neutrons that move at speeds comparable to those of air molecules at room…

A: Given: Speed of neutron = 691 m/s. And the mass of neutron = 1.675 × 10-27 Kg.

Q: Calculate the energy per mole of photons in kilojoules that has a frequency of 8.21 x 1012 sec-1 .

A: Since the frequency of each photon is given And we know that the energy of photon is given by E =…

Q: What is the frequency of the photon emitted from a Hydrogen atom's electron when it transitions from…

Q: What is the energy in kJ of a mole of photons associated with red light of wavelength 7.00 × 102 nm?

A: The energy of any photon is related to wavelength as, => E = hcλ where E = energy of each photon…

Q: A laser pointer used in the classroom emits light at 5950 Å, at a power of 4.00 mW. (One watt is the…

A: The expression to calculate the number of photons is given by, Number of photons = Total…

Q: Calculate the wavelength of the photon that would be released during a transition from n = 3 to n =…

Q: What is the wavelength of a photon if the energy is 7.73 × 10⁻¹⁹ J? (h = 6.626 × 10⁻³⁴ J • s)

A: Energy of photon is given by the formula -

Q: Calculate the wavelength in meters of electromagnetic radiation that has a frequency of 1.29 × 10⁸…

Q: What is the frequency of a photon with a=n energy of 2.00 x 10-16 J

A: Given: Energy = 2.00 x 10-16 J

Q: What is the de Broglie wavelength of an electron traveling at a 4.56×106 m/s? The mass of an…

Q: Calculate the energy of a photon in units of kJ/mol when it is emitted with a wavelength of 97.2nm.

A: The energy of a photon = hv The energy of 1 mole of photon = hv * NA Where, h is planks…

Q: An electron in a hydrogen atom jumps from n=7 to n = 5 and emits a photon. What is the wavelength of…

A: Given , nfinal= 5 ninitial=7 R=1.097×107 m-1 Wavelength =?

Q: An argon ion laser puts out 5.0 W of continuous power at a wavelength of 532 nm. The diameter of the…

Q: The blue color of the sky results from the scattering of sunlight by air molecules. The blue light…

Q: What is the wavelength of the light emitted when the electron in a hydrogen atom undergoes a…

Q: Compare the wavelength of an electron (mass = 9.11 x 10-31 kg) travelling at a speed of 1.0 x 106…

A: Given that two particles one is small and the other is bigger. The Dual behaviour is explained by…

Q: Determine the energy, in J, of a photon with a wavelength of 339nm. (h=6.626 x 10^-34 J * s and…

A: Given Wavelength = 339 nm 1 nm = 1× 10-9 meter 339 nm = 339 × 10-9 meter…

Q: Determine the energy, in J, of a photon with a wavelength of 351 nm. (h = 6.626 × 10⁻³⁴ J • s and c…

A: Given that: wavelength = 351 nm = 351×10-9 m h = 6.626 × 10⁻³⁴ J.s c = 3.00 × 10⁸ m/s To find,…

Q: If a laser emits 5.0 x 1019 photons per second and transfers a total of 80.58 J of energy over 2.06…

A: Given: A laser emits 5.0 x 1019 photons per second. The amount of energy transferred = 80.58 J in…

Concept explainers

Quantum Chemistry

Quantum chemistry deals with the properties of chemical systems and their reactions. The branch of chemistry which is more concerned with quantum chemistry is physical chemistry. It is a more sophisticated field of theoretical physics which is concerned towards the application of physical concepts towards various chemical aspects such as, formation of atoms, chemical structure descriptions, chemical bond strength, hybridization, conjugation etc. Quantum chemistry mainly studies the various states i.e., ground state, excited state, transition states of the individual atoms or molecules taking place during any chemical reaction. The laws of motion explained by various scientists, which are termed as “classical mechanics” were not acceptable in terms of electrons, protons, atoms, light etc. Thus, a new theory named “quantum mechanics” emerged to understand the basic framework of various atomic and subatomic particles.

Question

Calculate the energy (in joules) of a photon with a wavelength of 5.00 × 103 nm
Planck's constant is 6.626 X 10-34 J.s.: c = %v; E=hv; speed of light =c = 3.00 X 10° m/s;
v = frequency; =
wavelength
fiauration for iodine.

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Introduction and Principles of Quantum Theory

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

This laser emits green light with a wavelength of 533 nm. (a) What is the energy, in joules, of one photon of light at this wavelength? (b) If a particular laser produces 1.00 watt (W) of power (1 W = 1 J/s), how many photons are produced each second by the laser?
What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon energy? What does a photon energy unit of a joule equal?
Calculate the energy per mole of photons (in kJ/mol) for red light with a wavelength of 700 nm. Calculate the energy per mole of photons (in kJ/mol) for UV-B light with a wavelength of 300 nm. How many times more energetic is this UV-B than this red light?
(a) Calculate the frequency and the wavelength of the line for the n = 6 to n = 4 transition. (b) Is this wavelength longer or shorter than that of the n = 7 to n = 4 transition?
6.86 An excited He+ ion returns to the ground state by emitting a series of three photons, with wavelengths of 26 nm, 469 nm, and 1014 nm. The process is represented in the energy level diagram below. Which arrow (A, B, or C) in the diagram represents the 1014-nm light?
A particular transition of the rubidium atom emits light whose frequency is 3.84 1014 Hz. (Hz is the abbreviation for hertz, which is equivalent to the unit/s, or s1.) Is this light in the visible spectrum? If so, what is the color of the light? (See Figure 7.5.)
Show that the value of the Rydberg constant per photon, 2.179 1018 J, is equivalent to 1312 kJ/mol photons.
An FM radio station broadcasts at a frequency of 101.3 MHz. What is the wavelength, in meters and nanometers, of this radiation?
A bright violet line occurs at 435.8 nm in the emission spectrum of mercury vapor. What amount of energy, in joules, must be released by an electron in a mercury atom to produce a photon of this light?
Potassium atoms in a flame emit light as they undergo transitions from one energy level to another that is 4.91019J lower in energy. Calculate the wavelength of light emitted and, by referring to Figure 4.3, predict the color visible in the flame.
A hydrogen atom in the ground stale absorbs a photon whose wavelength is 95.0 nm. The resulting excited atom then emits a photon of 1282 nm. What are the regions of the electromagnetic spectrum for the radiations involved in these transitions? What is the principal quantum number of the final state resulting from the emission from the excited atom?
Light with a wavelength of 405 nm fell on a strontium surface, and electrons were ejected. If the speed of an ejected electron is 3.36 105 m/s, what energy was expended in removing the electron from the metal? Express the answer in joules (per electron) and in kilojoules per mole (of electrons).