To calculate the standard enthalpy change for the transition of water from ice at -10C to liquid water at 25C, we need to consider three steps:1. Heating the ice from -10C to 0C2. Melting the ice at 0C3. Heating the liquid water from 0C to 25CThe balanced chemical equation for the phase transition is:H2O s -> H2O l Step 1: Heating the ice from -10C to 0Cq1 = mcTwhere q1 is the heat required, m is the mass of water, c is the specific heat capacity of ice 2.09 J/gC , and T is the change in temperature 10C .q1 = m 2.09 J/gC 10CStep 2: Melting the ice at 0Cq2 = mHfuswhere q2 is the heat required and Hfus is the enthalpy of fusion for water 6.01 kJ/mol or 6.01 J/g .q2 = m 6.01 J/gStep 3: Heating the liquid water from 0C to 25Cq3 = mcTwhere q3 is the heat required, c is the specific heat capacity of liquid water 4.18 J/gC , and T is the change in temperature 25C .q3 = m 4.18 J/gC 25CThe total enthalpy change q_total is the sum of the enthalpy changes for each step:q_total = q1 + q2 + q3q_total = m 2.09 J/gC 10C + m 6.01 J/g + m 4.18 J/gC 25C Since we are looking for the standard enthalpy change, we can divide q_total by the mass m to get the enthalpy change per gram:H = 2.09 J/gC 10C + 6.01 J/g + 4.18 J/gC 25C H = 20.9 J/g + 6.01 J/g + 104.5 J/gH = 131.41 J/gSo, the standard enthalpy change for the transition of water from ice at -10C to liquid water at 25C is 131.41 J/g.