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Thermochemical Equations. Sam Wickert , Emily Szabo , Mikey Milici. What are thermochemical equations?. Themochemical Equations are chemical equations that include the enthalpy change of a reaction. CaO (s ) + H 2 O(l) → Ca (OH) 2 (s) + 65.2 kJ

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thermochemical equations

Thermochemical Equations

Sam Wickert, Emily Szabo, MikeyMilici

what are thermochemical equations
What are thermochemical equations?
  • Themochemical Equations are chemical equations that include the enthalpy change of a reaction.

CaO(s) + H2O(l) → Ca(OH)2(s) + 65.2 kJ

(Heat is givenoff, an exothermic Reaction)

  • Enthalpy is the heat content of a system at constant pressure. The heat released or absorbed by a reaction at constant pressure is the same as the change in enthalpy (∆H).
heat of reaction
Heat of Reaction
  • The heat of reaction is the enthalpy change for the chemical equation exactly as it is written.
  • These are usually reported as ∆H, which is equal to the heat flow at constant pressure.

CaO(s) + H2O(l) → Ca(OH)2(s) ∆H = -65.2 kJ

(Heat is given off, an exothermic Reaction)

  • Standard conditions are that the reaction is carried out at 101.3 kPa and that the reactants and products are in their usual physical states at 25˚C.
endothermic thermochemical equations
Endothermic Thermochemical Equations
  • Along with the previous examples of Exothermic thermochemical equations, other thermochemical equations may absorb heat from the surroundings.

2NaHCO3(s) + 129 kJ → Na2CO3(s) + H2O(g) + CO2(g)

  • Remember that ∆H is positive for endothermic reactions, therefore the above reaction can be written as:

2NaHCO3(s) → Na2CO3(s) + H2O(g) + CO2(g) ∆H = 129 kJ

heat of combustion
Heat of Combustion
  • The heat of combustion is the heat of reaction for the complete burning of one mole of a substance.
  • Example: burning 1 mol of methane releases 890 kJ of heat.
  • See full list of most common on page 570.