Data Table 2: Final Results Metal used: Trial 1 Trial 2 Trial 3 Mass of metal (g) 34.14g 28.76g 31.569 Mass of water (g) 29.03g 28.68g 27.33g Initial temperature of water ("C) 23.00C 22.00C 22.00C Initial temperature of metal ("C) 26.4C 25.3C 50.000 Final temperature of water ("C) 74.20 90.4C 32.000 Final temperature of metal ("C) 90.4C 96.00C Name: Specific Heat of a Metal Lab Dale: Per. Analysis and Calculations: Show your work including significant figures and appropriate units in order to receive FULL credit 1. Knowing your initial temperatures and final temperatures, calculate At for both the metal and water. Trial 1 Trial 2 Trial 3 Water: At t 74.2-23.00 51.1 C 90.2-22.00-68.2 32.00-22.00 10.00 C Metal: Al- 94.7-26.4 68.3 C 90.4-25.3 65.1C 96.00-50.00 46.00C 2. Knowing that the specific heat of water = 4.184 Jig "C, calculate the heat gained by the water using the equation q-mxsx At. Do this for all three trials. Show your work neatly. Trial 1 Q (29.03)(4.18451.1) 6206.6J Trial 3 Q (28.68) (4.184) (68.2) -8160.9J Q (27.33) (4.184) (10.00) -1143.4 J 3. Based on the Law of Conservation of Energy, calculate the heat lost by the metal: (-Heat Lost by the Metal Heat Gained by the Water) - your work neatly. Do this for al three trials. Show Trial 1 Trial 2 100 g x 4.18 Jig°C 5°C 2090 J 150 g x 4.18 J/g°C x 4°C = 2508 J -2090 J Trial 3 200 g x 4.18 Jig°C 3°C 2508 J 2508 J -2508 J 2090J/50 gx20 °C -2.09 Jig°C 2508 J/60 gx 18°C 2.32 J/g' C Specific Heat of a Metal Lab Name: Date: Per. 2508J/70 gx15 °C 2.39 Jig°C 2.09-2.15/2.15 x100-2.79% 2.32-2.15/2.15× 100% =7.91% 239-2.15/ 2.15 x 100% = 11.16% 4. Knowing the heat lost by the water, calculate the specific heat of the metalls) using the equation: sq/ (mx At). Do this for all three trials. Show your work neatly. Trial 1 74.2 degrees Celsius - 23.0 degrees Celsius = 51.2 degrees Celsius q 29.03 grams 4.18 Jig C 51.2 degrees Celsius = 6211.92 74.2 degrees Celsius - 23.0 degrees Celsius = 51.2 degrees Celsius q-29.03 grams 4.18 Jig C 51.2 degrees Celsius = 6211.92 Joules 94.7 degrees Celsius - 26.4 degrees Celsius 68.3 degrees Celsius Trial 2 6211.92 Joules/(34.14 grams *68.3 degrees Celsius) = 2.65 Jig°C 28.68 grams 27.33 grams Trial 3 Change in temperature of water = 32.0 degrees Celsius - 22.0 degrees Celsius 10.0 degrees Celsius Change in temperature of water = q 27.33 grams 4.18 Jig°C* 90.4 degrees Celsius - 22.0 degrees Celsius = 68.4 degrees Celsius q-28.68 grams 4.18 J/g C 68.4 degrees Celsius = 8183.95 Joules 90.4 degrees Celsius-25.3 degrees Celsius 65.1 degrees Celsius 8183.95 Joules (28.76 grams * 65.1 degrees Celsius) -4.41 Jig C 10.0 degrees Celsius 1142.94 Joules 96.0 degrees Celsius - 50.0 degrees Celsius 46.0 degrees Celsius 1142.94 Joules/(31.55 grams 46.0 degrees Celsius) 0.79 Jig°C 5. Using the accepted specific heat value for the metal(s) to calculate % error. Show your work. Use the internet to google the accepted value in Jig"C. Trial 1 Trial 2 Trial 3