Measuring and Expressing Enthalpy Changes. Copyright Pearson Prentice Hall. Measuring and Expressing Enthalpy Changes. Calorimetry

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1 Measuring and Expressing Enthalpy Changes A burning match releases heat to its surroundings in all directions. How much heat does this exothermic reaction release? You will learn to measure heat flow in chemical and physical processes by applying the concept of specific heat. 1 of 33 Measuring and Expressing > What basic concepts apply to calorimetry? 2 of 33 1

2 is the precise measurement of the heat flow into or out of a system for chemical and physical processes. 3 of 33 In calorimetry, the heat released by the system is equal to the heat absorbed by its surroundings. Conversely, the heat absorbed by a system is equal to the heat released by its surroundings. 4 of 33 2

3 The insulated device used to measure the absorption or release of heat in chemical or physical processes is called a calorimeter. 5 of 33 Constant-Pressure Calorimeters The heat content of a system at constant pressure is the same as a property called the enthalpy (H) of the system. 6 of 33 3

4 Constant-Volume Calorimeters experiments can be performed at a constant volume using a bomb calorimeter. 7 of 33 SAMPLE PROBLEM 8 of 33 4

5 Practice Problems for Sample Problem Problem Solving Solve Problem 13 with the help of an interactive guided tutorial. 9 of 33 Measuring and Expressing > How can you express the enthalpy change for a reaction in a chemical equation? 10 of 33 5

6 Measuring and Expressing > In a chemical equation, the enthalpy change for the reaction can be written as either a reactant or a product. 11 of 33 A chemical equation that includes the enthalpy change is called a thermochemical equation. 12 of 33 6

7 The heat of reaction is the enthalpy change for the chemical equation exactly as it is written. 13 of 33 Exothermic Reaction 14 of 33 7

8 Endothermic Reaction 15 of 33 SAMPLE PROBLEM of 33 8

9 Practice Problems for Sample Problem 17.3 Problem Solving Solve Problem 15 with the help of an interactive guided tutorial. 17 of of 33 9

10 The heat of combustion is the heat of reaction for the complete burning of one mole of a substance. 19 of The change in temperature recorded by the thermometer in a calorimeter is a measurement of. A. the enthalpy change of the reaction in the calorimeter. B. the specific heat of each compound in a calorimeter. C. the physical states of the reactants in a calorimeter. D. the heat of combustion for one substance in a calorimeter. 20 of 33 10

11 2. For the reaction: CaO(s) + H 2 O(l) Ca(OH) 2 (s), H = kj. This means that 62.5 kj of heat is during the process. A. absorbed B. destroyed C. changed to mass D. released 21 of How much heat is absorbed by 325 g of water if its temperature changes from 17.0 C to 43.5 C? The specific heat of water is 4.18 J/g C. A kj B kj C kj D. 360 kj 22 of 33 11

12 4. Which of the following is a thermochemical equation for an endothermic reaction? A. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) kj B kj + 2H 2 O(l) 2H 2 (g) + O 2 (g) C. CaO(s) + H 2 O(l) Ca(OH) 2 (s) kj D. H 2 (g) + O 2 (g) H 2 O(g) kj 23 of Oxygen is necessary for releasing energy from glucose in organisms. How many kj of heat are produced when 2.24 mol glucose reacts with an excess of oxygen? C 6 H 12 O 6 (s) + 6O 2 (g) 6CO 2 (g) + 6H 2 O(g) kj/mol A kj B kj C kj D kj 24 of 33 12

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