The enthalpy change for the oxidation of butane, C4H10, is measured by calorimetry. C4H10 (g) + 13/2 O2 (g) → 4 CO2 (g) + 5 H₂O(l) ΔΗ° - 2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO₂ (g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = kJ/mol

The enthalpy change for the oxidation of butane, C4H10, is measured by calorimetry. C4H10 (g) + 13/2 O2 (g) → 4 CO2 (g) + 5 H₂O(l) ΔΗ° - 2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO₂ (g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = kJ/mol

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For which one of the following is the enthalpy of the reaction the same as the enthalpy of formation? A) 2 H (g) + Se (s) → H:Se (g) B) KOH (s) → K*(aq) + OH- (aq) C) 2 Fe (s) + 3 Cl2 (g) → 2 FeCl3 (s) D) Ni (s) + ½ O2 (g)- NiO (s)
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Use Hess’s law to calculate the enthalpy change for the reaction WO3(s) + 3H2(g) —> W(s) +3H2O(g) from the following data: 2W(s) + 3O2(g) —> 2 WO3(s) H=-1685.4 2H2(g) + O2(g) —> 2H2O(g) H=-477.84
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