Ch.7 - Quantum MechanicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: How much energy (in kJ) do 3.00 moles of photons, all with a wavelength of 675 nm, contain?A) 532 kJ B) 177 kJ C) 238 kJ D) 418 kJ E) 354 kJ

Solution: How much energy (in kJ) do 3.00 moles of photons, all with a wavelength of 675 nm, contain?A) 532 kJ B) 177 kJ C) 238 kJ D) 418 kJ E) 354 kJ

Problem

How much energy (in kJ) do 3.00 moles of photons, all with a wavelength of 675 nm, contain?

A) 532 kJ 

B) 177 kJ 

C) 238 kJ 

D) 418 kJ 

E) 354 kJ

Solution

We´re asked to determine the energy (in kJ) of 3.00 moles of photons and a wavelength of 675 nm.


Remember that the Energy and the frequency of a photon are related by the following equation:

E=

Where

E is the energy of the photon (in J)

h is the Planck’s constant (h = 6.626x10-34 J*s)

ν is the frequency of the photon (in s-1)

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