Answered: Calculate the energy of 1.215 moles of…

Calculate the energy of 1.215 moles of light with a wavelength of 188.334 nm. 6.02 x 1023 things = 1.00 mol(things) c = 3.00 x 108 m/sec h = 6.626 x 10-34 J sec

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

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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 of 1.215 moles of light with a wavelength of 188.334 nm.

6.02 x 10²³ things = 1.00 mol(things) c = 3.00 x 10⁸ m/sec

h = 6.626 x 10^-34 J sec

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