The standard heat of formation, ΔH∘fΔHf∘, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0ΔHf∘=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘fΔHf∘ (kJ/molkJ/mol) NO(g)NO(g) 90.2 O2(g)O2(g) 0 NO2(g)NO2(g) 33.2 Then the standard heat of reaction for the overall reaction is ΔH∘rxn===ΔH∘f(products)2(33.2)−114 kJ−−ΔH∘f(reactants)[2(90.2)+0] The combustion of ethene, C2H4C2H4, occurs via the reaction C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)C2H4(g)+3O2(g)→2CO2(g)+2H2O(g) with heat of formation values given by the following table: Substance ΔH∘fΔHf∘ (kJ/molkJ/mol) C2H4C2H4 (g)(g) 52.47 CO2(g)CO2(g) −−393.5 H2O(g)H2O(g) −−241.8 Calculate the enthalpy for the combustion of 1 mole of ethene. Express your answer to four significant figures and include the appropriate units. View Available Hint(s) ΔH∘rxnΔHrxn∘ =
The standard heat of formation, ΔH∘fΔHf∘, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0ΔHf∘=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘fΔHf∘ (kJ/molkJ/mol) NO(g)NO(g) 90.2 O2(g)O2(g) 0 NO2(g)NO2(g) 33.2 Then the standard heat of reaction for the overall reaction is ΔH∘rxn===ΔH∘f(products)2(33.2)−114 kJ−−ΔH∘f(reactants)[2(90.2)+0] The combustion of ethene, C2H4C2H4, occurs via the reaction C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)C2H4(g)+3O2(g)→2CO2(g)+2H2O(g) with heat of formation values given by the following table: Substance ΔH∘fΔHf∘ (kJ/molkJ/mol) C2H4C2H4 (g)(g) 52.47 CO2(g)CO2(g) −−393.5 H2O(g)H2O(g) −−241.8 Calculate the enthalpy for the combustion of 1 mole of ethene. Express your answer to four significant figures and include the appropriate units. View Available Hint(s) ΔH∘rxnΔHrxn∘ =
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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The standard heat of formation, ΔH∘fΔHf∘, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0ΔHf∘=0. Heat of formation values can be used to calculate the enthalpy change of any reaction.
Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g)
with heat of formation values given by the following table:
| Substance | ΔH∘fΔHf∘ (kJ/molkJ/mol) |
| NO(g)NO(g) | 90.2 |
| O2(g)O2(g) | 0 |
| NO2(g)NO2(g) | 33.2 |
Then the standard heat of reaction for the overall reaction is
ΔH∘rxn===ΔH∘f(products)2(33.2)−114 kJ−−ΔH∘f(reactants)[2(90.2)+0]
The combustion of ethene, C2H4C2H4, occurs via the reaction
C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)C2H4(g)+3O2(g)→2CO2(g)+2H2O(g)
with heat of formation values given by the following table:
| Substance | ΔH∘fΔHf∘ (kJ/molkJ/mol) |
| C2H4C2H4 (g)(g) | 52.47 |
| CO2(g)CO2(g) | −−393.5 |
| H2O(g)H2O(g) | −−241.8 |
Calculate the enthalpy for the combustion of 1 mole of ethene.
Express your answer to four significant figures and include the appropriate units.
View Available Hint(s)
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ΔH∘rxnΔHrxn∘ =
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