A 250 g sample of molten lead is held at its melting point (327 °C). The molar enthalpy of fusion of lead is 4.77 kJ mol⁻¹, and its molar mass is 207.2 g mol⁻¹. Two equal cooling pulses each remove 1.50 kJ of energy, but only 85 % of that energy actually leaves the lead due to heat losses. After both pulses, what mass of the lead sample (in g) remains in the liquid state?