Part A Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change Calculate the enthalpy change, AH, for the process in which 36.9 g of water is converted from liquid at 9.4 "C to vapor at 25.0 "C. For water, AHvap = 44.0 kJ/mol at 25.0 "C and C; = 4.18 J/(g . "C) q = m . C: . AT for H2O(1). where C is specific heat and m is mass. Express your answer to three significant figures and include the appropriate units. Heat can also be transferred at a constant temperature when there is a change in state. For a View Available Hint(s) process that involves a phase change q = n . AH where, n is the number of moles and AH is the HA 1 ? enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and AH = Value Units enthalpy changes for water and ice Substance Specific heat AH [J/(g . "C)] (kJ/mol) Submit water 4.18 44.0 ice 2.01 6.01 Part B How many grams of ice at -18.1 "C can be completely converted to liquid at 15.3 "C if the available heat for this process is 5.73x103 kJ ? For ice, use a specific heat of 2.01 J/(g . "C) and AHfus = 6.01kJ/mol Express your answer to three significant figures and include the appropriate units. View Available Hint(s)