**Photoelectric Effect Problem**It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (in nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? (Planck's constant, *h* = 6.626 x 10⁻³⁴ Js)**Options:**- 725 nm- 471 nm- 165 nm- 233 nmThis problem involves calculating the maximum wavelength of light that can overcome the work function (energy required to remove an electron) of a metal, which is provided in energy per mole. You will need to convert this energy into energy per photon using Avogadro's number, and then apply the photoelectric equation to find the wavelength.

Given: Energy = 254 kJ/mol h = 6.626×10-34 J.s

It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? (h = 6.626 x 10*34 Js) %3D O 725 O 471 O 165 O 233

It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? (h = 6.626 x 10*34 Js) %3D O 725 O 471 O 165 O 233

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes a transition…

A: The Rydberg equation gives the wavelength λ for the transitions: where R = the Rydberg constant (…

Q: In a hypothetical 1-electron element that is not H, removing an electron (thus bringing it to the…

A: Given that the energy needed for the n=1 to n=∞ transition is 412 kJ/mol and the energy for the n=2…

Q: he energy required to remove electrons from elemental cesium is 376 kJ/mol. Which wavelength(s) of…

A: energy = hcλ where h = Plank's constant c = velocity of light λ = wavelength

Q: What wavelength (in nanometers) of light is emitted when an electron in a hydrogen atom falls from…

A: Here, we have to calculate the wavelength (in nanometers) of light that is emitted when an electron…

Q: 8. Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of…

Q: How many electrons in an atom could have these sets of quantum numbers? n = 3 18 electrons n = 4, l…

A: There are four quantum numbers. Principal quantum number(n) which says the shell number, Azimuthal…

Q: 2. When an electron in the n = 5 level of a H atom emits a photon of wavelength 1281 nm, to what…

Q: Ionization energy is defined as the minimum energy required to remove an electron from the ground…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: A ground state hydrogen atom absorbs a photon of light having a wavelength of 94.92 nm. It then…

Q: Calculate the wavelength of light (in nm) emitted when an electron in a hydrogen atom makes a…

Q: The energy required to remove electrons from elemental sodium is 496 kJ/mol. What is the threshold…

A: From Planck's quantum equation E = h νowhere E = work function = 496 x 103 J /mol h = 6.625 x…

Q: An electron in the hydrogen atom can drop from the n=3 level to the n=2 level.What is the Energy of…

Q: 2. The green light emitted by a stoplight has a wavelength of 505 nm. What is the frequency of this…

A: As per Q&A guidelines of portal I solve first question because it comes under multiple question…

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: For He+ ion, calculate the wavelength of the light that is emitted upon the electron's transition…

A: This numerical is related to Rydberg formula which is used to determine wavelength of light emitted…

Q: The work function of an element is the energy required to re- move an electron from the surface of…

A: The maximum wavelength that remove an electron from an atom is 427.94 nm. that is approximately…

Q: It requires 3.69 x 10^-19 J of energy to eject an electron from potassium metal. Calculate the…

Q: What is the wavelength, in nanometers, of light with an energy content of 1979 kJ/mol

A: We have: Energy= E= 1979 KJ/mol We need to calculate the wavelength of light (in nm). Using the…

Q: For doubly ionized lithium (only one electron left), what is the wavelength of the emitted photon as…

A: Given :- ion from which electron undergoes transition = Li2+ transition of electron takes place…

Q: N₂(g) + hv→ N₂(g) + e¯ 1. What is the maximum wavelength of a photon needed to ionize N₂ if the…

A: Maximum wavelength is calculated by planck's equation

Q: Green light can have energy of 3.88 x 10^-19 J. Calculate the wavelength of this light.

A: Energy of the electron is the product of Plank's constant and frequency. One mole of electrons…

Q: a) Calculate the wavelength of light (in nm) produced when an electron moves from n= 8 to n=3 in a…

Q: Calculate the energy of a photon emitted when an electron in a hydrogen atom undergoes a transition…

A: Since you have posted two questions , as per guidelines we can answer one per session . If you want…

Q: The minimum frequency of light needed to eject electrons from a metal is called the threshold…

Q: 8. An electron in a He* ion relaxes from n = 7 to n = 4. Calculate the wavelength (in units of…

Q: Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a…

A: Given data is as follows: The transition of an electron to n1 = 1 The transition of an electron from…

Q: The energy of the n=2 He* ions is the same as the energy of the n-1 orbital of the hydrogen atom.…

Q: Determine the wavelength of light emitted when an electron drops from n=4 to n=1 in a hydrogen atom.…

A: we have to calculate the wavelength of light emitted due to the transition from n = 4 to n = 1

Q: Calculate energy of photons emitted by 0.312 g Na with the wavelength 587 nm. Na = 22.99 g/ mole…

A: Photon energy is the energy carried by a single photon. Energy associated with one photon can be…

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

Q: Calculate the wavelength, in nanometers, of the spectral line produced when an electron in a…

Q: A minimum of 221.9 kJ/mol is required to remove an electron from a(n) potassium metal surface. What…

Q: Consider an atom of hydrogen that absorbs light of a wavelength 955.8 nm. What is the energy, in J,…

A: Given that, a hydrogen atom absorbs a light of wavelength 955.8 nm. So, the wavelength is λ = 955.8…

Q: a. What is the maximum number of electrons that can be identified with the following set of quantum…

A: The maximum number of electrons for each set of quantum numbers will be-Explanation:Step 1: Step 2:…

Q: wavelength

Q: 1. calculate the emission wavelength in nm of the photon that is emitted when an electron in a…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: The red line in the hydrogen spectrum corresponds to a transition from the energy level n=3 to the…

Q: If a minimum of 454.4 kJ/mol is required to remove electrons from Ru atoms on a surface of a sample…

Q: Thomson also experimented with shining ultraviolet light at metal electrodes, such as zinc, to…

A: To calculate the maximum wavelength of light that can be used to eject an electron from zinc given…

Q: An energy of 6.9 x 10^-19 J/atom is required to cause an iron atom on a metal surface to lose an…

A: The answer to the following question is given as:

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

**Photoelectric Effect Problem**

It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (in nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect? (Planck's constant, *h* = 6.626 x 10⁻³⁴ Js)

**Options:**
- 725 nm
- 471 nm
- 165 nm
- 233 nm

This problem involves calculating the maximum wavelength of light that can overcome the work function (energy required to remove an electron) of a metal, which is provided in energy per mole. You will need to convert this energy into energy per photon using Avogadro's number, and then apply the photoelectric equation to find the wavelength.

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

Trending now

This is a popular solution!

Step by step

Solved in 4 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

The hydrogen spectrum is complex. When a hydrogen atom absorbs a photon, it causes the electron to experience a transition to a higher energy level. Likewise, when the transition occurred from higher to lower energy level, emission spectra obtained. The wavelength of light associated with the n 2 to n = 1 electron transition in the hydrogen spectrum is 3.146 x 10- m. What coefficient should this wavelength be multiplied to obtain the wavelength associated with the same electron transition in the B4+ ion? %3D Select one: O a. 1/18 O b. 1/25 O c. 1 O d. 1/9 O e. 1/5
Which element would be more likely the wavelength of light: 423 K+ Sr2+ Ca2+ Cu(II) Na+ Li+
The kinetic energy of an electron ejected from the surface of a metal is 4.68 x 10-19 J. Calculate the wavelength of the light needed to produce the kinetic energy mentioned above if the threshold frequency to eject the electron is 1.82 x 1014 s-1. 650. nm 820. nm 520. nm 425 nm 338 nm
a) When a voltage is applied and current passes through sodium vapor, electrons are raised from the 3s to the 3p orbitals (energy levels). When this occurs, the atom is said to be in what state?When one of these electrons falls back to the 3s orbital, it emits a photon with a wavelength of 590 nm. What color of light is emitted from a lamp that uses sodium vapor?
An atom is ionized so that it has only one electron. When the electron drops from the n = 3 shell to the n = 1 shell, an X-ray of wavelength 121.97 pm is emitted. What is the atomic number?
The energy levels the electron can occupy in the Li2+ ion can be calculated using the energy level equation. A Li2+ ion emitted a photon with a wavelength of 72.9 nm to reach an energy level with n=2. What was the value of n for its initial energy level?
The threshold frequency vo describes the smallest light frequency capable of ejecting electrons from a metal. Determine the minimum energy Eo of a photon capable of ejecting electrons from a metal with vo = 2.66 x 10¹4 s-¹. Eo = What is the maximum kinetic energy KEclection of electrons ejected from this metal by light with a wavelength of 255 nm? KEclectron =
2. What is the wavelength of light emitted when an electron in a hydrogen atom transitions from the n=5 to the n= 3 level?
show your solution.
Consider the atom whose electron configuration is [Ne]3s^2 3p^1 Write the one-or two-letter symbol for the element. also how many unpaired electrons are there in the ground state of this atom?
For Fe25+ ion, calculate the wavelength of the light that is emitted upon the electron's transition from n=4 to n=3.
Calculate the wavelength?