Question
Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn, for the reaction in bold...
Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn, for the reaction in bold below given the following chemical steps and their respective enthalpy changes. Show ALL work!
2 C(s) + H2(g) → C2H2(g) ΔH°rxn = ?
1. C2H2(g) + 5/2 O2(g) → 2CO2 (g) + H2O (l) ΔH°rxn = -1299.6 kJ
2. C(s) + O2(g) → CO2 (g) ΔH°rxn = -393.5 kJ
3. H2(g) + ½ O2(g) → H2O (l) ΔH°rxn = -285.8 kJ
Homework Answers
Answer #1
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We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction...
We can use Hess's law to calculate enthalpy changes that cannot
be measured. One such reaction is the conversion of methane to
ethylene: 2CH4(g)⟶C2H4(g)+2H2(g) Calculate the ΔH∘ for this
reaction using the following thermochemical data:
CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g)
ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ
2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l ΔH∘=−3120.8kJ
9. Use the following experimentally derived combustion data to calculate the standard molar enthalpy of formation...
9. Use the following experimentally derived combustion
data to calculate the standard molar enthalpy of formation
(ΔH°f ) of liquid methanol (CH3OH) from its
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2 CH3OH(l) + 3 O2(g) → 2
CO2(g) + 4 H2O(l)
ΔH°rxn = −1452.8 kJ
C(graphite) + O2(g) →
CO2(g)
ΔH°rxn = −393.5 kJ
2 H2(g) + O2(g) → 2
H2O(l)
ΔH°rxn = −571.6 kJ
(1) −238.7 kJ/mol (2) 487.7
kJ/mol (3) −548.3 kJ/mol
(4) 20.1 kJ/mol
(5) 47.1 kJ/mol
We can use Hess's law to calculate enthalpy changes that cannot be measured. One such reaction...
We can use Hess's law to calculate enthalpy changes that cannot
be measured. One such reaction is the conversion of methane to
ethylene:
2CH4(g)⟶C2H4(g)+2H2(g)
Part A
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thermochemical data:
CH4(g)+2O2(g)⟶CO2(g)+2H2O(l)
ΔH∘=−890.3kJ
C2H4(g)+H2(g)⟶C2H6(g)
ΔH∘=−136.3kJ
2H2(g)+O2(g)⟶2H2O(l)
ΔH∘=−571.6kJ
2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l)
ΔH∘=−3120.8kJ
Express your answer to four significant figures and include the
appropriate units.
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= -241.8 kJ
calculate the enthalpy change for the following reaction:
4 H2 (g) + 3 C (s)→ C3H8 (g)
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the same whether the process takes place in one or in several
steps."
It is important to recall the following rules:
When two reactions are added, their enthalpy values are
added.
When a reaction is reversed, the sign of its enthalpy value
changes.
When the coefficients of a reaction are multiplied by a factor,
the enthalpy value is multiplied by that same factor.
Part A
Calculate...
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Given tha delta hydrogen = -393.5 kJ for the rxn.: C(s) +O2(g) -> CO2(g), and given...
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1/2O2(g) -> H2O(l), and given
that delta hydrogen = -84.7 kJ for the rxn .: 3H2(g) +2C
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calculate the dleta hydrogen for the rxn C2H6(g) + 3 1/2O2(g)
-> 2CO2(g) + 3HO(l)
Delta hydrogen = kJ
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