Part A The standard heat of formation, A H°, 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 A H° = 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) with heat of formation values given by the following table: Af H° (kJ mol¹) Substance NO(g) 90.2 O2(g) NO(g) 0 33.2 For which of the following reactions is A, H° equal to Ar H° of the product(s)? You do not need to look up any values to answer this question. Check all that apply. ▷ View Available Hint(s) Na(s)+ Fa(g) → NaF(s) D CO(g)+ ;O2(g) → CO2(g) Na(s)+ F₂(1) NaF(s) 2Na(s)+F2(g) → 2NaF(s) C(s)+ O2(g) → CO2 (g) Then the heat of formation for the overall reaction is A,H A H°(products)- ΣnA H°(reactants) 2(33.2) -114 kJ mol-1 (2(90.2)+0 Submit Part B The combustion of ethene, C2H4, occurs via the reaction with heat of formation values given by the following table: Substance C2H4 (g) A H° (kJ mol¹) 52.47 CO₂(s) -393.5 H₂O(g) -241.8 C2H4(g)+302(g)2CO2(g) + 2H2O(g) Calculate the enthalpy for the combustion of ethene. Express your answer to one decimal place and include the appropriate units.
Part A The standard heat of formation, A H°, 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 A H° = 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) with heat of formation values given by the following table: Af H° (kJ mol¹) Substance NO(g) 90.2 O2(g) NO(g) 0 33.2 For which of the following reactions is A, H° equal to Ar H° of the product(s)? You do not need to look up any values to answer this question. Check all that apply. ▷ View Available Hint(s) Na(s)+ Fa(g) → NaF(s) D CO(g)+ ;O2(g) → CO2(g) Na(s)+ F₂(1) NaF(s) 2Na(s)+F2(g) → 2NaF(s) C(s)+ O2(g) → CO2 (g) Then the heat of formation for the overall reaction is A,H A H°(products)- ΣnA H°(reactants) 2(33.2) -114 kJ mol-1 (2(90.2)+0 Submit Part B The combustion of ethene, C2H4, occurs via the reaction with heat of formation values given by the following table: Substance C2H4 (g) A H° (kJ mol¹) 52.47 CO₂(s) -393.5 H₂O(g) -241.8 C2H4(g)+302(g)2CO2(g) + 2H2O(g) Calculate the enthalpy for the combustion of ethene. Express your answer to one decimal place and include the appropriate units.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.10: Standard Formation Enthalpies
Problem 4.18CE
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Transcribed Image Text:Part A
The standard heat of formation, A H°, 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 A H° = 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)
with heat of formation values given by the following table:
Af H°
(kJ mol¹)
Substance
NO(g)
90.2
O2(g)
NO(g)
0
33.2
For which of the following reactions is A, H° equal to Ar H° of the product(s)?
You do not need to look up any values to answer this question.
Check all that apply.
▷ View Available Hint(s)
Na(s)+ Fa(g) → NaF(s)
D CO(g)+ ;O2(g) → CO2(g)
Na(s)+ F₂(1) NaF(s)
2Na(s)+F2(g) → 2NaF(s)
C(s)+ O2(g) → CO2 (g)
Then the heat of formation for the overall reaction is
A,H A H°(products)- ΣnA H°(reactants)
2(33.2)
-114 kJ mol-1
(2(90.2)+0
Submit
Part B
The combustion of ethene, C2H4, occurs via the reaction
with heat of formation values given by the following table:
Substance
C2H4 (g)
A H°
(kJ mol¹)
52.47
CO₂(s)
-393.5
H₂O(g)
-241.8
C2H4(g)+302(g)2CO2(g) + 2H2O(g)
Calculate the enthalpy for the combustion of ethene.
Express your answer to one decimal place and include the appropriate units.
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