To calculate the standard enthalpy change for the phase transition of water from ice to liquid at 25C and 1 atm pressure, we need to consider two steps: 1. Heating the ice from -273.15C 0 K to 0C 273.15 K 2. Melting the ice at 0C 273.15 K Step 1: Heating the ice from -273.15C to 0CThe heat capacity of ice is approximately 2.09 J/gK. To calculate the enthalpy change for heating the ice, we can use the formula:H = m C Twhere H is the enthalpy change, m is the mass of the substance, C is the heat capacity, and T is the temperature change.Assuming 1 mole of ice 18.015 g , the enthalpy change for heating the ice is:H1 = 18.015 g 2.09 J/gK 273.15 K - 0 K = 18.015 g 2.09 J/gK 273.15 K 10,340 JStep 2: Melting the ice at 0CThe enthalpy of fusion for water melting ice to liquid is 6.01 kJ/mol.H2 = 6.01 kJ/mol 1000 J/kJ = 6010 JNow, we can add the enthalpy changes for both steps to find the total enthalpy change for the phase transition of water from ice to liquid at 25C and 1 atm pressure:H_total = H1 + H2 = 10,340 J + 6010 J 16,350 JTherefore, the standard enthalpy change for the phase transition of water from ice to liquid at 25C and 1 atm pressure is approximately 16,350 J/mol.