Calculate the heat of atomization (see previous problem) of C 2 H 3 Cl, using the average bond energies in Table 9.3.

hey everyone in this example we need to calculate heat of atomization for di chloral, floral methane. And we're going to first begin by recalling that our heat of atomization is going to equal two times the bond energy of our two carbon chlorine bonds in the molecule, Added to two times the bond energy of our two chlorine. Or sorry, carbon flooring bonds in our molecules. So this should just be carbon here. So looking these values up, we can say that our entropy of atomization is going to equal two times the bond energy of a carbon chlorine. Single bond equal to 339 kg joules per mole in our textbooks Which is then added to two times the carbon flooring single bonds in our molecule Which have a bond energy of inner textbooks as 485 kg joules per mole. So this is going to give us a value equal to 1648 kg joules per mole as our final answer for our heat of atomization of our dick, laurel floor, methane. So this will be our final answer. To complete this example. If you have any questions, please leave them down below. Otherwise, I'll see everyone in the next practice video

Ch.9 - Chemical Bonding I: The Lewis Model

All textbooks

Tro 4th Edition

Ch.9 - Chemical Bonding I: The Lewis Model

Problem 112

Previous problem

Next problem

Chapter 9, Problem 112

Calculate the heat of atomization (see previous problem) of C₂H₃Cl, using the average bond energies in Table 9.3.

Verified step by step guidance

Step 1: Identify the bonds present in the molecule. In C2H3Cl, there are 1 C=C bond, 2 C-H bonds, 1 C-Cl bond, and 1 C-C bond.

Step 2: Look up the average bond energies for each type of bond in Table 9.3. Let's denote them as BE(C=C), BE(C-H), BE(C-Cl), and BE(C-C) respectively.

Step 3: Calculate the total energy required to break all the bonds in the molecule. This is done by multiplying the number of each type of bond by its bond energy and adding all these values together. The formula is: Total Energy = BE(C=C) + 2*BE(C-H) + BE(C-Cl) + BE(C-C).

Step 4: The heat of atomization is the energy required to break all the bonds in the molecule, so it is equal to the total energy calculated in step 3.

Step 5: The unit of the heat of atomization will be the same as the unit of bond energy, usually kilojoules per mole (kJ/mol).

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Heat of Atomization

The heat of atomization is the amount of energy required to convert one mole of a substance into its individual atoms in the gas phase. This value is crucial for understanding the stability of molecules and the energy changes involved in chemical reactions. It can be calculated using bond energies, which represent the strength of the bonds between atoms in a molecule.

Bond Energies

Bond energies are the average energy required to break a specific type of bond between atoms in a molecule. These values are typically expressed in kilojoules per mole (kJ/mol) and vary depending on the types of atoms involved and their bonding environment. By using average bond energies, one can estimate the total energy change associated with breaking all the bonds in a molecule, which is essential for calculating the heat of atomization.

C2H3Cl Molecular Structure

C2H3Cl, or vinyl chloride, has a specific molecular structure that includes carbon, hydrogen, and chlorine atoms. Understanding its structure is vital for identifying the types of bonds present, such as C-H, C-C, and C-Cl bonds. This knowledge allows for the correct application of bond energies to calculate the heat of atomization, as each bond type contributes differently to the overall energy required to separate the molecule into individual atoms.

Recommended video:

Molecular Formula

Related Practice

The azide ion, N₃^-, is a symmetrical ion, all of whose contributing resonance structures have formal charges. Draw three important contributing structures for this ion.

2356

views

Textbook Question

List the following gas-phase ion pairs in order of the quantity of energy released when they form from separated gas-phase ions. List the pair that releases the least energy first. Na⁺ F^-, Mg²⁺F^-, Na⁺O^2-, Mg²⁺O^2-, Al³⁺O^2-.

The heat of atomization is the heat required to convert a molecule in the gas phase into its constituent atoms in the gas phase. The heat of atomization is used to calculate average bond energies. Without using any tabulated bond energies, calculate the average C–Cl bond energy from the following data: the heat of atomization of CH₄ is 1660 kJ/mol, and the heat of atomization of CH₂Cl₂ is 1495 kJ/mol.

A compound composed of only carbon and hydrogen is 7.743% hydrogen by mass. Propose a Lewis structure for the compound.

994

views

Textbook Question

A compound composed of only carbon and chlorine is 85.5% chlorine by mass. Propose a Lewis structure for the compound.

2478

views

Calculate the heat of atomization (see previous problem) of C2H3Cl, using the average bond energies in Table 9.3.

Verified Solution

Key Concepts

Heat of Atomization

Bond Energies

C2H3Cl Molecular Structure

Calculate the heat of atomization (see previous problem) of C₂H₃Cl, using the average bond energies in Table 9.3.