Measuring Energy Changes in a Chemical Reaction Calorimetry 2015.

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Measuring Energy Changes in a Chemical Reaction Calorimetry 2015

Key concept: EVERY chemical reaction either releases energy to the surroundings (exothermic reactions) OR absorbs energy from the surrounding (endothermic reactions) We cannot measure the energy changes in the chemical reaction (the system) BUT we can easily measure the energy changes in the surroundings If we assume that: heat lost/gained by the system = heat gained/lost by the surroundings then we can experimentally determine the energy changes in chemical reactions

Key concept: To measure the heat gained/lost by the surroundings we need a device called a calorimeter Calorimeters can be as simple as a beaker filled with water or as sophisticated as a bomb calorimeter

Coffee cup calorimeterBomb calorimeter

Example 1: What amount of heat is released when 2.56 g of ethane burns? Assumption: All heat lost by the reaction goes into the copper calorimeter and the water. Given: The temperature of both the copper calorimeter and the water increase by 70.3 o C The specific heat capacity of water is 4.18 J/g o C The specific heat capacity of copper is J/g o C

q = mcΔT (can only used for surroundings) Heat gained by the water: q = (450g)(4.18J/g o C)(70.3 o C) = J Heat gained by the copper calorimeter: q = (25.0g)(0.385 J/g o C)(70.3 o C) = J Heat lost by the reaction q rxn = q water + q copper = J = kJ This is called the “heat of the reaction”

What amount of heat is released when 1 mole of ethane burns?(units will be kJ/mol) When 2.56 g of ethane burns, kJ of energy is released OR kJ of energy is released when ____ mol of ethane is burned Amount of heat/mol = kJ/ mol = 1561 kJ/mol

Now that the units are “standardized” we call this energy change “enthalpy of the reaction”. Rather than using the symbol “q”, we use the symbol “ΔH”. Since heat has been lost by the system, it is an _________ reaction and we indicate this loss by using the (–)ve sign. Therefore: ΔH = kJ/mol

Example 2: What is the heat of the reaction when 10.0g of propane burns? Given: The temperature of both the calorimeter and water increases from 25.0 o C to 90.5 o C The heat capacity of the calorimeter is 2.0 kJ/ o C The specific heat capacity of water is 4.18 J/g o C

q = mcΔT and q = C ΔT q water = q calorimeter = q rxn = q water + q calorimeter

What is the molar enthalpy of combustion of propane? ________ mol of propanol releases _________ kJ of energy Therefore ΔH = _________ = ________ kJ/mol

Example 3: What is the molar enthalpy of dissolution (dissolving) of NaOH? Given: Heat absorbed by coffee cup = 0 J Water temperature increases from 25 o C to 38.3 o C q water = q rxn = q water = n NaOH = ΔH =