The average bond enthalpy of the C − C bond is to be calculated. Concept introduction: The bond enthalpy is the energy required to break a bond of one mole of a substance. The change of enthalpy is defined as the difference of the enthalpy of the products and the enthalpy of the reactants, multiplied by their respective stoichiometric coefficients.

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Definition Definition Number that is expressed before molecules, ions, and atoms such that it balances out the number of components present on either section of the equation in a chemical reaction. Stoichiometric coefficients can be a fraction or a whole number and are useful in determining the mole ratio among the reactants and products. In any equalized chemical equation, the number of components on either side of the equation will be the same.

Chapter 8, Problem 125AP

Interpretation Introduction

Interpretation:

The average bond enthalpy of the C−C bond is to be calculated.

Concept introduction:

The bond enthalpy is the energy required to break a bond of one mole of a substance.

The change of enthalpy is defined as the difference of the enthalpy of the products and the enthalpy of the reactants, multiplied by their respective stoichiometric coefficients.

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Use average bond energies together with the standard enthalpy of formation of C( g) (718.4 kJ/mol) to estimate the standard enthalpy of formation of gaseous benzene, C6H6( g). (Remember that average bond energies apply to the gas phase only.) Compare the value you obtain using average bond energies to the actual standard enthalpy of formation of gaseous benzene,82.9 kJ/mol. What does the difference between these two values tell you about the stability of benzene?

The average bond enthalpy for C−H is 413 kJ/mol. 413 kJ of energy is required to break a mole of CH into atoms: CH(g)→C(g)+H(g), ΔH=413 kJ Using this information, and your answer from Part A, calculate the enthalpy change of the reaction from Part B. That is, calculate the energy required to break only the carbon-carbon bonds in benzene. PART A ANSWER ΔH∘rxn = 5535.1 kJ.. PART B ANSWER C6H6(g)→6CH(g)

In chemical reactions, heat is converted into chemical energy (the potential energy stored in chemical bonds) or vice versa. Bond energy is the energy required to break one mole of the bond in the gas phase. Since it takes energy to break a bond, bond energies are always positive. Conversely, energy is released when bonds are formed. Thus, the enthalpy change for a reaction can be approximated from Part A Calculate the bond energy per mole for breaking all the bonds in methane, CH4. ΔΗ Σ(ΔΗ breaking) + Σ(ΔΗ forming) Express your answer to four significant figures and include the appropriate units. where H represents bond energies for the breaking (positive bond energy) or forming (negative bond energy) of a bond and Hrxn represents the overall enthalpy for the • View Available Hint(s) reaction. Use the table to answer questions about bond energies. HẢ Bond energy Bond (kJ/mol ) Value Units AHCH, = C-C 347 C=C 611 Submit Сн 414 C-O 360 Part B C=OinCO2 799 O-0 142 Calculate the bond…

Answer 2

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Definition Definition Number that is expressed before molecules, ions, and atoms such that it balances out the number of components present on either section of the equation in a chemical reaction. Stoichiometric coefficients can be a fraction or a whole number and are useful in determining the mole ratio among the reactants and products. In any equalized chemical equation, the number of components on either side of the equation will be the same.

Chapter 8, Problem 125AP

Interpretation Introduction

Interpretation:

The average bond enthalpy of the C−C bond is to be calculated.

Concept introduction:

The bond enthalpy is the energy required to break a bond of one mole of a substance.

The change of enthalpy is defined as the difference of the enthalpy of the products and the enthalpy of the reactants, multiplied by their respective stoichiometric coefficients.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 3

Question

Definition Definition Number that is expressed before molecules, ions, and atoms such that it balances out the number of components present on either section of the equation in a chemical reaction. Stoichiometric coefficients can be a fraction or a whole number and are useful in determining the mole ratio among the reactants and products. In any equalized chemical equation, the number of components on either side of the equation will be the same.

Chapter 8, Problem 125AP

Interpretation Introduction

Interpretation:

The average bond enthalpy of the C−C bond is to be calculated.

Concept introduction:

The bond enthalpy is the energy required to break a bond of one mole of a substance.

The change of enthalpy is defined as the difference of the enthalpy of the products and the enthalpy of the reactants, multiplied by their respective stoichiometric coefficients.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Definition Definition Number that is expressed before molecules, ions, and atoms such that it balances out the number of components present on either section of the equation in a chemical reaction. Stoichiometric coefficients can be a fraction or a whole number and are useful in determining the mole ratio among the reactants and products. In any equalized chemical equation, the number of components on either side of the equation will be the same.

Chapter 8, Problem 125AP

Interpretation Introduction