Part (c) please. The answer is meant to be fusH 6.2 kJ mol1

When ice is in equilibrium with a solution of ethylene glycol in water, such that Mw(s) = pw(l), the depression of the water freezing point, AT = (T T*), due to the presence of ethylene glycol in the water can be approximated as = = AT = -XEG RT+2 Afus H Equation (1) where Xeg is the mole fraction of ethylene glycol, T* is the melting point of pure water, and Afus H is the enthalpy of fusion of ice. (b) Show how the ideal solution model can be used to derive the equation above for AT, noting clearly any further assumptions. You may find it helpul to use the Gibbs-Helmholtz equation, and to note that ln(1 x) ~ -x for x