Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

9. Quantum Mechanics

The Energy of Light

General Chemistry

9. Quantum Mechanics

The Energy of Light

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Multiple Choice

How much energy (in kJ) do 3.0 moles of photons, all with a wavelength of 655 nm, contain?

912 kJ

1200 kJ

750 kJ

550 kJ

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Verified step by step guidance

First, understand that the energy of a photon can be calculated using the equation: \( E = \frac{hc}{\lambda} \), where \( E \) is the energy of a photon, \( h \) is Planck's constant \( (6.626 \times 10^{-34} \text{ J s}) \), \( c \) is the speed of light \( (3.00 \times 10^8 \text{ m/s}) \), and \( \lambda \) is the wavelength in meters.

Convert the given wavelength from nanometers to meters. Since 1 nm = \( 1 \times 10^{-9} \) m, the wavelength \( \lambda = 655 \text{ nm} \) is equivalent to \( 655 \times 10^{-9} \text{ m} \).

Substitute the values of \( h \), \( c \), and \( \lambda \) into the energy equation to find the energy of a single photon: \( E = \frac{(6.626 \times 10^{-34} \text{ J s})(3.00 \times 10^8 \text{ m/s})}{655 \times 10^{-9} \text{ m}} \).

Calculate the energy for one photon using the above expression. This will give you the energy in joules for one photon.

To find the total energy for 3.0 moles of photons, multiply the energy of one photon by Avogadro's number \( (6.022 \times 10^{23} \text{ photons/mole}) \) and then by 3.0 moles. Convert the result from joules to kilojoules by dividing by 1000.