Enthalpy of a Reaction

    Cards (10)

    • Enthalpy (H)
      • "energy change"
      • quantifies the heat flow into or out of the system in a process the occurs at constant pressure
      • tells us about the "heat content" of a system
    • Enthalpy of Reactions (ΔH_rxn)
      • heat transferred in a chemical reaction held at constant pressure
      • the difference between the enthalpies of the products and the enthalpies of the reactants
      • ΔH_rxn = H(products) - H(reactants)
      • ΔH > 0 (+): endothermic
      • ΔH < 0 (-): exothermic
    • Enthalpy Changes unit: kJ/mol
    • Interpreting Thermochemical Equations
      1.) Physical states of all the reactants and products must be specified.
      2.) Reversing a reaction would result in a change in sign but the magnitude of ΔH remains the same.
      3.) Multiplying both sides of the equation by a factor n, would also change ΔH by the same factor n.
      4.) The stoichiometric coefficients always refer to the number of moles of a substance.
    • Standard Molar Enthalpy of Formation (ΔHof)
      Standard states:
      • natural state of a substance at 1 atm
      • an element in its standard state has an ΔHof = 0 kJ/mol
    • Standard Molar Enthalpy of Formation (ΔHof)
      Formation Reaction:
      • a reaction where one mole of a substance is formed from elements in their standard states
      It is a formation reaction if it satisfied all of the following:
      • both reactants are in their standard states
      • only 1 mole of the product is produced
    • Standard Enthalpy of Reaction (ΔHo_rxn)
      • enthalpy of a reaction carried out at 1 atm
      • ΔHo_rxn = ∑(nΔHof products) - ∑(nΔHof reactants)
    • For calculating ΔHo_rxn:
      Direct Method
      • use when only one equation/reaction is given
      Indirect method
      • for multiple step reactions
    • Hess Law:
      • the overall enthalpy change in converting reactants to products is the same, regardless if it took place in one step or multiple steps reaction
    • Hess law:
      1. Balance the chemical reaction.
      2. Align the reactants and products in the same position as the one-step (main) process.
      3. Manipulate the coefficients align with the main process.
      4. Cancel like substances in reactants and products.
      5. Add the enthalpies.
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