Thermochemistry and Glucose Metabolism Quiz
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Thermochemistry and Glucose Metabolism Quiz

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Questions and Answers

What is the value of ΔHrxn for the reaction of maleic acid to fumaric acid at 298 K?

  • 23.3 kJ mol−1
  • -15.0 kJ mol−1
  • -23.3 kJ mol−1 (correct)
  • -7.6 kJ mol−1

    • Which of the following is the correct balanced equation for glucose metabolism?

  • C6H12O6 + 3 O2 → 6 CO2 + 3 H2O
  • C6H12O6 + O2 → 6 CO2 + 6 H2O
  • C6H12O6 + 6 O2 → 6 CO2 + 6 H2O (correct)
  • C6H12O6 + 2 O2 → 6 CO2 + 3 H2O

    • What is the standard enthalpy of formation for glucose (C6H12O6) at 305 K?

  • −393.5 kJ mol−1
  • −285.8 kJ mol−1
  • 0 kJ mol−1
  • −1273.0 kJ mol−1 (correct)

    • What is the enthalpy of formation for water (H2O) at 305 K?

    <p>−285.8 kJ mol−1</p> Signup and view all the answers

    If the enthalpy of formation of diatomic oxygen (O2) is considered, what is its value?

    <p>0 kJ mol−1</p> Signup and view all the answers

    How is ΔHrxn calculated for the conversion of maleic acid to fumaric acid?

    <p>ΔHrxn = Hf(fumaric) - Hf(maleic)</p> Signup and view all the answers

    When calculating enthalpy changes, what is the significance of using standard conditions?

    <p>It standardizes the enthalpy values based on 298 K and 1 atm pressure.</p> Signup and view all the answers

    In the context of thermochemistry, what does the term 'enthalpy of formation' specifically refer to?

    <p>The heat change during the formation of one mole of a compound from its elements.</p> Signup and view all the answers

    Study Notes

    Thermochemistry Problems

    • Determine the enthalpy of reaction (ΔHrxn) for the conversion of Maleic acid to Fumaric acid.
      • The enthalpy of formation of Fumaric acid is -807.6 kJ/mol.
      • The enthalpy of formation of Maleic acid is -784.4 kJ/mol.
      • The enthalpy change for the reaction can be calculated by subtracting the enthalpy of formation of the reactants from the enthalpy of formation of the products.
      • ΔHrxn = ΔHf°(products) - ΔHf°(reactants)
      • ΔHrxn = (-807.6) - (-784.4) = -23.3 kJ/mol

    Glucose Metabolism

    • Glucose is metabolized in the presence of oxygen to produce carbon dioxide and water.
      • The balanced chemical equation for this reaction is: C6H12O6 + 6O2 → 6CO2 + 6H2O
      • The enthalpy of formation (ΔHf°) for glucose is -1273.0 kJ/mol.
      • The enthalpy of formation for oxygen is 0 kJ/mol.
      • The enthalpy of formation for water is -285.8 kJ/mol.
      • The enthalpy of formation for carbon dioxide is -393.5 kJ/mol.
      • The enthalpy change for the reaction can be calculated using the following equation:
        • ΔHrxn = Σ ΔHf°(products) - Σ ΔHf°(reactants)
        • ΔHrxn = [6(-393.5) + 6(-285.8)] - [-1273.0 + 6(0)] = -2803.0 kJ/mol

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    Description

    Test your knowledge on thermochemistry concepts, including the calculation of enthalpy changes for reactions like the conversion of Maleic acid to Fumaric acid. Additionally, explore glucose metabolism and its enthalpy of formation. Challenge yourself with these important biochemical reactions!

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