As more mass is added it raises the temperature of the water. C Work mwater AT Use this equation to calculate the specific heat of the water for each trail in part 2. Take note that if the beaker contains 296 ml of water, it will also be 296 g of water. Mass of water (t Record your values in the table below: Mass (kg) Work (Joules) Change in Temperature (C) Specific Heat of Water (-) 114 3.91 5.8 7.45 9.37 11.34 12.61 Part 3: The Specific Heat of Water When James Joules performed this experiment in the 19th century, he was primarily trying to determine the amount of energy required to raise the temperature of a specific amount of water. Today, we refer to this quantity as the specific heat for a material. Using data from part 2 of this lab, you are going to experimentally determine the specific heat of water. 1. Transfer the mass and change in temperature values from your part 2 table to the table below. 2. Determine the work done by each mass in part 2 and record in the table below. The work done is equal to the potential energy that the mass contained prior to falling. W = PE=mgh The height that each mass falls in part 2 is 3.9 m, while g (the acceleration due to gravity) has a value of 9.8 m 3. Recall that energy is conserved. As such, the work done on the system will equal the heat gained by the system. Work (done by falling mass) Heat (gained by water) 169 217 273 330 367 Work = = mwater CAT Solving for the specific heat (c), we get... 4. Calculate the average specific heat of water value for this lab and record below: 5. What does this number represent?