Chapter 5 Thermochemistry Terms I • Thermochemistry – Study of – • Kinetic Energy – Energy of • Potential Energy – Energy of Units of E • JOULE • Calorie vs. calorie – 1 Cal = – 1 cal is the amount of heat necessary to raise the temperature of 1 g of water 1oC • 1 cal = J Terms II • Force –A • Work – Energy used to move an object –W= • Energy – Capacity to do First Law of Thermodynamics • Energy •ΔE = Equation II •ΔE = • q = heat in or heat out of system • w = work done on or by the system Practice • Calculate the change in the internal energy of the system for a process in which the system absorbs 140 J of heat from the surroundings and does 85 J of work on the surroundings. Endothermic Reaction • Process when a system • Gets • ΔH > Exothermic Reaction • Process when a system • Gets • ΔH < State Function • Describes the condition of a system • Does not matter how the system got there • For example… ENTHALPY • Heat… – • Represented by • Is a Enthalpy Equation • ΔH = Hfinal – Hinitial = qp • P indicates constant pressure Enthalpy of Reaction • ΔHrxn = H(products) – H(reactants) • 2H2O (g) 2H2 (g) + O2 (g) ΔH = • 2H2 (g) + O2(g) 2H2O(g) ΔH = Return Rules for Enthalpy and RXNS 1. Enthalpy is an extensive property 2. Enthalpy for a reaction 3. Enthalpy change depends on state of reactants and products Practice • 2Mg(s) + O2(g) 2MgO(s) ΔH=-1204 kJ • Is this • How much heat is transferred when 2.40 g of Mg are reacted? • How many grams of MgO are produced during an enthalpy change of 96.0 kJ? Continued • 2Mg(s) + O2(g) 2MgO(s) ΔH=-1204 kJ • How many kJ of heat are absorbed when 7.50 g of MgO(s) are decomposed into magnesium and oxygen at constant pressure? Calorimetry • The study of • Heat capacity (C): – Temperature change of an object as it – Amount of heat required to – Greater heat capacity means… Calorimetry • Molar heat capacity (Cmolar) • Specific heat capacity (Cp) – • Equation: Calorimetry • What is the heat required to raise 400.00 g of water by 34.50oC? • What is the heat lost when 200.00 g of iron changes from 115.50 oC to 22.00 oC? Calorimetry • Large beds of rocks are used in some solar heated homes to store heat. Assume that the specific heat of rock is 0.082 J/g-K. Calculate the quantity of heat absorbed by 50.0 kg of rocks if their temperature increases by 12.0 oC Flashback… • Law of conservation of energy (First law of thermodynamics): – – Calorimetry • You have heated a 55.00 g piece of iron, Cp = 0.385 J/g-K, to 200.00 oC. You then put the iron into water in a calorimeter. There are 300.00 g of water at 22.00 oC. What is the final temperature of the mixture? Calorimetry • In the calorimetry lab you will be mixing an acid and a base and studying the temperature changes. • You mix 35.00 mL each of 1 M HCl and 1 M NaOH in a calorimeter. The temperature increases from 21.0 to 27.5 oC. What is the enthalpy change for the reaction in kJ/mol HCl? Hess’s Law Enthalpy of Formation • Energy change for the formation • Symbolized by Hf • Tables are for standard conditions – 1 atm – 25oC • Appendix C Enthalpy of Formation • Units for Hof are in • Magnitude depends on state • 2H2(g) + O2(g) 2 H2O(l) Hof = -285.8 • 2H2(g) + O2(g) 2 H2O(g) Hof = 241.8 Enthalpy of Formation • By definition: the standard enthalpy of formation of the most stable form of ANY element is 0 kJ/mol • Hof C(s) = 0 • Hof H2(g) = 0 Enthalpy of RXN • Horxn = Σn Hof (products) - Σm Hof (reactants)