Textbook Question
Write an equation for the formation of each compound from its elements in their standard states, and find ΔH°rxn for each in Appendix IIB. d. CH3OH(l)
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Ch.6 - Thermochemistry
Chapter 6, Problem 87
Use standard enthalpies of formation to calculate ΔH°rxn for the reaction: CO(g) + H2O(g) → H2(g) + CO2(g)
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Identify the standard enthalpy of formation (ΔH°f) for each compound involved in the reaction: CO(g), H2O(g), H2(g), and CO2(g). These values are typically found in a table of standard enthalpies of formation.
Write the balanced chemical equation for the reaction: CO(g) + H2O(g) → H2(g) + CO2(g).
Apply the formula for calculating the standard enthalpy change of the reaction (ΔH°rxn): ΔH°rxn = Σ(ΔH°f of products) - Σ(ΔH°f of reactants).
Substitute the standard enthalpy of formation values into the formula: ΔH°rxn = [ΔH°f(H2) + ΔH°f(CO2)] - [ΔH°f(CO) + ΔH°f(H2O)].
Calculate the sum of the enthalpies of formation for the products and the reactants separately, then subtract the sum for the reactants from the sum for the products to find ΔH°rxn.
Related Practice
Textbook Question
Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4 according to the equation: N2H4 (l) + N2O4 (g) → 2 N2O (g) + 2 H2O (g) Calculate ΔH°rxn for this reaction using standard enthalpies of formation.
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Textbook Question
Pentane (C5H12) is a component of gasoline that burns according to the following balanced equation: C5H12(l) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) Calculate ΔH°rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of liquid pentane is –146.8 kJ/mol.)
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Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. a. C2H4(g) + H2(g) → C2H6(g)
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Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. c. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
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Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. d. Cr2O3(s) + 3 CO(g) → 2 Cr(s) + 3 CO2(g)
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