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Compare your answer from Exercise 72 of Chapter 3 to the ∆H value calculated from standard enthalpies of formation in Appendix 4. Explain any discrepancies. ….. 72. Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction: Use tabulated values of bond engines(Table 3-3) to estimate ∆ E for this reaction

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 7, Problem 113AE
Textbook Problem
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Compare your answer from Exercise 72 of Chapter 3 to the ∆H value calculated from standard enthalpies of formation in Appendix 4. Explain any discrepancies.

…..

72. Acetic acid is responsible for the sour taste of vinegar. It can be manufactured using the following reaction:

Chapter 7, Problem 113AE, Compare your answer from Exercise 72 of Chapter 3 to the H value calculated from standard enthalpies

Use tabulated values of bond engines(Table 3-3) to estimate ∆E for this reaction

Interpretation Introduction

Interpretation: The comparative estimation of calculated enthalpy change and internal energy change of the given reaction should be explained.

Hess's Law:

Standard enthalpy of formation:

  • The change in enthalpy that associate with the formation of one mole of a product from its pure elements, with all substances in its standard states is called as a standard enthalpy of formation.
  • Formula:

    ΔHfnpΔH°f(products)-nrΔH°f(reactants)......(1)

  • Internal energy change of a reaction is given as,
  • Internal energy change ΔE= Bond broken energy - Bond formation energy

    ΔE=Dbroken-Dformed......(2)

  • The internal energy change is equal to enthalpy change in the gas phase reactions.

Explanation of Solution

Explanation

Record data from given:

CH3OH(g)+CO(g)CH3COOH(l)

C-Cbondenergy=347kJ/molC-Obondenergy=358kJ/mol CdoublebondO=745 kJ/molC triple bondO=1072kJ/mol

The given reactions and bond energies arerecorded as shown above.

To calculate the internal energy change of the given reactions.

ΔE=1072+358kJ-(347+745+358)=-20 kJ

  • Thegiven bond energies are plugging in to above equation 2to get the internal energy change of the reactions.
  • Internal energy change of reaction (a) = -20kJ .

To calculate the enthalpy change ΔΗ of given reactions

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Chapter 7 Solutions

Chemistry: An Atoms First Approach
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