Heat, q, is energy transferred between a system and its Part A surroundings. For a process that involves a temperature change Calculate the enthalpy change, H, for the process in which 33.5g of water is converted from liquid at 10.1C to vapor at 25.0C. For water, Hvap=44.0kJ/mol at 25.0C and Cs=4.18J/(gC) for H2O(l). where Cs 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 process that involves a phase change q=nH where, n is the number of moles and H is the enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and enthalpy changes for water and ice. Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature How many grams of ice at 27.0C can be completely converted to liquid at 12.5C if the available heat for this process is 4.80103kJ ? change For ice, use a specific heat of 2.01J/(gC) and Hfus=6.01kJ/mol. q=mCsT where Cs 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 process that involves a phase change q=nH where, n is the number of moles and H is the enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and enthalpy changes for water and ice. E OneDrive Screenshot saved