Chapter 17 Thermochemistry 17.2 Measuring and Expressing 17.1 The Flow of Energy 17.2 Measuring and Expressing Enthalpy Changes 17.3 Heat in Changes of State 17.4 Calculating Heats of Reaction Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Enthalpy Change in a Calorimetry Experiment Sample Problem 17.3 Enthalpy Change in a Calorimetry Experiment When 25.0 mL of water containing 0.025 mol HCl at 25.0°C is added to 25.0 mL of water containing 0.025 mol NaOH at 25.0°C in a foam-cup calorimeter, a reaction occurs. Calculate the enthalpy change (in kJ) during this reaction if the highest temperature observed is 32.0°C. Assume that the densities of the solutions are 1.00 g/mL and the volume of the final solution is equal to the sum of the volumes of the reacting solutions. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations How can you express the enthalpy change for a reaction in a chemical equation? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations In a chemical equation, the enthalpy change for the reaction can be written as either a reactant or a product. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations In the equation describing the exothermic reaction of calcium oxide and water, the enthalpy change can be considered a product. CaO(s) + H2O(l) → Ca(OH)2(s) + 65.2 kJ Calcium oxide is one of the components of cement. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations A chemical equation that includes the enthalpy change is called a thermochemical equation. CaO(s) + H2O(l) → Ca(OH)2(s) + 65.2 kJ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction The heat of reaction is the enthalpy change for the chemical equation exactly as it is written. Heats of reaction are reported as ΔH. The physical state of the reactants and products must also be given. The standard conditions are that the reaction is carried out at 101.3 kPa (1 atm) and 25°C. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction Each mole of calcium oxide and water that reacts to form calcium hydroxide produces 65.2 kJ of heat. CaO(s) + H2O(l) → Ca(OH)2(s) ΔH = –65.2 kJ In exothermic processes, the chemical potential energy of the reactants is higher than the chemical potential energy of the products. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction Baking soda (sodium bicarbonate) decomposes when it is heated. This process is endothermic. 2NaHCO3(s) + 85 kJ → Na2CO3(s) + H2O(l) + CO2(g) The carbon dioxide released in the reaction causes muffins to rise while baking. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction 2NaHCO3(s) + 85 kJ → Na2CO3(s) + H2O(l) + CO2(g) Remember that ΔH is positive for endothermic reactions. Therefore, you can write the reaction as follows: 2NaHCO3(s) → Na2CO3(s) + H2O(l) + CO2(g) ΔH = 85 kJ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction The amount of heat released or absorbed during a reaction depends on the number of moles of the reactant involved. The decomposition of 2 mol of sodium bicarbonate requires 85 kJ of heat. Therefore, the decomposition of 4 mol of the same substance would require twice as much heat, or 170 kJ. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction To see why the physical state of the reactants and products must be stated, compare the following two equations. difference = 44.0 kJ H2O(l) → H2(g) + O2(g) ΔH = 285.8 kJ 1 2 H2O(g) → H2(g) + O2(g) ΔH = 241.8 kJ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Reaction To see why the physical state of the reactants and products must be stated, compare the following two equations. difference = 44.0 kJ H2O(l) → H2(g) + O2(g) ΔH = 285.8 kJ 1 2 H2O(g) → H2(g) + O2(g) ΔH = 241.8 kJ The vaporization of 1 mol of liquid water to water vapor at 25°C requires 44.0 kJ of heat. H2O(l) → H2O(g) ΔH = 44.0 kJ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Using the Heat of Reaction to Calculate Enthalpy Change Sample Problem 17.4 Using the Heat of Reaction to Calculate Enthalpy Change 2NaHCO3(s) + 85 kJ → Na2CO3(s) + H2O(l) CO2(g) Calculate the amount of heat (in kJ) required to decompose 2.24 mol NaHCO3(s). Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Combustion The heat of combustion is the heat of reaction for the complete burning of one mole of a substance. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Thermochemical Equations Heats of Combustion Small amounts of natural gas within crude oil are burned off at oil refineries. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) + 890 kJ This is an exothermic reaction. Burning 1 mol of methane releases 890 kJ of heat. The heat of combustion (ΔH) for this reaction is –890 kJ per mole of methane burned. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Heats of Combustion at 25°C Interpret Data Heats of Combustion at 25°C Substance Formula ΔH (kJ/mol) Hydrogen H2(g) –286 Carbon C(s, graphite) –394 Methane CH4(g) –890 Acetylene C2H2(g) –1300 Ethanol C2H6O(l) –1368 Propane C3H8(g) –2220 Glucose C6H12O6(s) –2808 Octane C8H18(l) –5471 Sucrose C12H22O11(s) –5645 Like other heats of reaction, heats of combustion are reported as the enthalpy changes when the reactions are carried out at 101.3 kPa and 25°C. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Which of the following thermochemical equations represents an endothermic reaction? A. Cgraphite(s) + 2 kJ Cdiamond(s) B. 2H2(g) + O2(g) 2H2O + 483.6 kJ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Which of the following thermochemical equations represents an endothermic reaction? A. Cgraphite(s) + 2 kJ Cdiamond(s) B. 2H2(g) + O2(g) 2H2O + 483.6 kJ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.