To calculate the standard enthalpy change for the transition of ice to water, we need to consider three steps:1. Heating the ice from -10 C to 0 C2. Melting the ice at 0 C3. Heating the water from 0 C to 50 CFirst, let's calculate the moles of water in 50 grams:moles = mass / molar mass = 50 g / 18 g/mol = 2.78 molStep 1: Heating the ice from -10 C to 0 Cq1 = mass specific heat capacity of ice Tq1 = 50 g 2.09 J/gC 0 - -10 Cq1 = 50 g 2.09 J/gC 10 Cq1 = 1045 JStep 2: Melting the ice at 0 CThe enthalpy of fusion for water is 6.01 kJ/mol. We will use this to calculate the energy required to melt the ice.q2 = moles enthalpy of fusionq2 = 2.78 mol 6.01 kJ/molq2 = 16.7 kJConvert to Joules:q2 = 16.7 kJ 1000 J/kJ = 16700 JStep 3: Heating the water from 0 C to 50 Cq3 = mass specific heat capacity of water Tq3 = 50 g 4.18 J/gC 50 - 0 Cq3 = 50 g 4.18 J/gC 50 Cq3 = 10450 JNow, we add up the energy for all three steps to find the total standard enthalpy change:Total enthalpy change = q1 + q2 + q3Total enthalpy change = 1045 J + 16700 J + 10450 JTotal enthalpy change = 28195 JThe standard enthalpy change for the transition of 50 grams of ice to water when heated from -10 C to 50 C is 28,195 Joules.