The energy required to dissociate the Cl2 molecule to Cl atoms is 239 kJ / mol Cl2. If the diss

Name: Problem 107, Chapter 7: General Chemistry
Uploaded: 2021-06-22T20:01:34-08:00
Duration: 1 min 25 s
Channel: Lottie Adams
Description: The energy required to dissociate the Cl2 molecule to Cl atoms is 239 kJ / mol Cl2. If the dissociation of a Cl2 molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength (in meters)?

step 1 And chlorine, so this is our group 7 halogen with 7 valence electrons. It's rather an electroneg

Question

The energy required to dissociate the $\mathrm{Cl}_{2}$ molecule to $\mathrm{Cl}$ atoms is $239 \mathrm{~kJ} / \mathrm{mol} \mathrm{Cl}_{2}$. If the dissociation of a $\mathrm{Cl}_{2}$ molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength (in meters)?

   The energy required to dissociate the $\mathrm{Cl}_{2}$ molecule to $\mathrm{Cl}$ atoms is $239 \mathrm{~kJ} / \mathrm{mol} \mathrm{Cl}_{2}$. If the dissociation of a $\mathrm{Cl}_{2}$ molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength (in meters)?

General Chemistry

Darrell Ebbing,… 9th Edition

Chapter 7, Problem 107

Instant Answer

Solved by Expert Lottie Adams

06/22/2021

Step 1

First, we need to convert the energy required to dissociate the Cl2 molecule from kJ/mol to Joules per molecule. We know that 1 mol contains Avogadro's number of molecules (6.022 x 10^23 molecules/mol), and 1 kJ = 1000 J. Energy per molecule = (239 kJ/mol) * Show more…

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The energy required to dissociate the $\mathrm{Cl}_{2}$ molecule to $\mathrm{Cl}$ atoms is $239 \mathrm{~kJ} / \mathrm{mol} \mathrm{Cl}_{2}$. If the dissociation of a $\mathrm{Cl}_{2}$ molecule were accomplished by the absorption of a single photon whose energy was exactly the quantity required, what would be its wavelength (in meters)?

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Key Concepts

Planck’s Equation

Planck’s equation, expressed as E = hc/?, links the energy of a photon to its wavelength through Planck's constant (h) and the speed of light (c). This equation is central in the study of quantum mechanics and electromagnetic radiation, establishing the relationship between energy and wave properties.

Molar to Single-Entity Energy Conversion

In many chemical processes, energy is given per mole of entities, but for photon interactions, the energy per individual photon is required. This conversion is achieved by dividing the molar energy by Avogadro’s number, allowing a transition from macroscopic to microscopic thermodynamic quantities.

Photon Energy

Photon energy refers to the discrete amount of energy carried by a photon, which is quantized as determined by quantum mechanics. It is foundational in understanding how light interacts with matter, with the energy of a photon being directly related to its frequency or inversely to its wavelength.

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