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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Ch.6 - Thermochemistry
Chapter 6, Problem 88
Use standard enthalpies of formation to calculate ΔH° for the reaction: C(s) + H2O(g) → CO(g) + H2(g).
Verified step by step guidance1
Identify the standard enthalpy of formation (ΔH_f°) for each substance involved in the reaction. Remember that the standard enthalpy of formation for any element in its standard state, such as C(s), is zero.
Write the balanced chemical equation for the reaction: C(s) + H2O(g) → CO(g) + H2(g).
Use the formula for calculating the standard enthalpy change of the reaction: ΔH° = Σ(ΔH_f° of products) - Σ(ΔH_f° of reactants).
Substitute the standard enthalpies of formation into the formula: ΔH° = [ΔH_f°(CO) + ΔH_f°(H2)] - [ΔH_f°(C) + ΔH_f°(H2O)].
Calculate the sum of the enthalpies of formation for the products and subtract the sum of the enthalpies of formation for the reactants to find ΔH° for the reaction.
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Textbook Question
Use standard enthalpies of formation to calculate ΔH°rxn for each reaction. d. N2O4(g) + 4 H2(g) → N2(g) + 4 H2O(g)