1. Practicing Calorimetry

2. At the end of this lesson, you will be able to 30–A1.4k write balanced equations for chemical reactions that include energy changes 30–A1.5k use and interpret H notation to communicate and calculate energy changes in chemical reactions 30–A1.6k predict the enthalpy change for chemical equations using standard enthalpies of formation

3. In calorimetry, we must assume that the calorimeter is an isolated system. Calculating Enthalpy Change

4. Calorimetry of Chemical Changes In a chemistry experiment, 4.24g of lithium chloride is dissolved in 100.0 mL of water at an initial temperature of 16.3 o C. The final temperature of the water was 25.1 o C. Determine the molar enthalpy of solution. (the energy released by the ionization)

5. All chemical changes involve potential energy changes so we must use

7. Calorimetry of Chemical Changes- example 2 In an aluminum calorimeter, 20.0 g of nitrogen was burned in oxygen to produce nitrogen monoxide. From the following information, find the molar heat of combustion. Write the answer as an product/reactant in a balanced reaction. In an aluminum calorimeter, 20.0 g of nitrogen was burned in oxygen to produce nitrogen monoxide. From the following information, find the molar heat of combustion. Write the answer as an product/reactant in a balanced reaction. – Mass of nitrogen burned– 20.0g – Mass of aluminum calorimeter– 70.37 g – Volume of water –500.0 mL – Initial temp– 72.60 o C – Final Temp—12.80 o C

9. Example 3: In an experiment to determine the accuracy of a calorimeter, a student combusted 3.75 g of ethane and found the temperature of 1.50L of water increased from 15.2 to 48.2. The accepted value for the enthalpy of combustion of ethane is - 1560.4kJ/mol Determine the experimental specific heat of water.

11. Determine the experiment error of the experiment. Complete the “Using Calorimetry Assignment”

12. Homework Complete the “Using Calorimetry Assignment” Complete the “Using Calorimetry Assignment”