15.3 Thermochemical Equations

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Presentation transcript:

15.3 Thermochemical Equations Pages 529 – 533

A. Thermochemical Equations A thermochemical equation is a balanced chemical equation that includes the physical states of all reactants and products, and energy change In a thermochemical equation, the enthalpy of change for the reaction can be written as either a reactant or a product

A. Thermochemical Equations How to write thermochemical equations: Endothermic (positive ΔH) 2NaHCO3(s)+ 129kJ Na2CO3(s) + H2O(g) + CO2(g) Exothermic (negative ΔH) CaO(s) + H2O(l) Ca(OH)2(s) + 65.2kJ

B. Thermochemical Equation Practice Write the thermochemical equation for the addition of oxygen gas to solid iron (III) if the ΔHrxn= -1652 kJ Fe(s) + O2(g)→ Fe2O3(s) + 1652 kJ Write the thermochemical equation for the decomposition of sulfur trioxide gas into sulfur dioxide gas and oxygen gas if the ΔHrxn= 198 kJ SO3(g) + 198 kJ → SO2 (g) + O2 (g) Exothermic 4 3 2 Endothermic 2 2

15.4 Hess’s Law Pages 534 – 540

A. Hess’s Law Hess’s law states that if you can add two or more thermochemical equations to produce a final equation for a reaction, then the sum of the enthalpy changes for the individual reactions is the enthalpy change for the final reaction 2S(s) + 3O2(g)  2SO3(g) H = ?

A. Hess’s Law

B. Hess’s Law Practice N2(s) + 2O2(g)  2NO2(g) H = ? Known: N2 (g) + O2(g)  2NO(g) H = -180 kJ 2NO(g) + O2(g)  2NO2(g) H = -112 kJ Build your equation:

B. Hess’s Law Practice 2H2O2(l)  2H2O(l) + O2(g) H = ? Known: 2H2(g) + O2(g)  2H2O(l) H = -572 kJ H2(g) + O2(g)  H2O2(l) H = -188 kJ Build your equation:

B. Hess’s Law Practice 2S(s) + 3O2(g)  2SO3(g) H = ? Known: S(s) + O2(g)  SO2(g) H = -297 kJ 2SO3(g)  2SO2(g) + O2(g) H = 198 kJ Build your equation:

B. Hess’s Law Practice 2B(s) + 3H2(g)  B2H6(g) H = ? Known: 2B (s) + 3/2O2(g)  B2O3(s) H = -1273 kJ B2H6(g) + 3O2(g)  B2O3 (s) + 3H2O (g) H = -2035 kJ H2 (g) + ½ O2(g)  H2O (l) H = -286 kJ H2O (l)  H2O (g) H = 44 kJ Build your equation: