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A piece of solid lead weighing38.4 g at a temperature of 315 Â°Cis placed in 384 g of liquid leadat a temperature of 372 Â°C. After a while, thesolid melts and a completely liquid sample remains. Calculate thetemperature after thermal equilibrium is reached, assuming no heatloss to the surroundings.

The enthalpy of fusion of solid lead isÎ”H_fus = 4.77 kJ/mol at its meltingpoint of 328 Â°C, and the molar heat capacities forsolid and liquid lead are C_solid =26.9 J/mol K and C_liquid =28.6J/mol K.
T_final =Â Â Â°C

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The amount of energy required q1 to heat 384 g of lead at 315 Cto 328 C CsolidmolesTWhere T final temperature initial temperature 328 C 315 C 13 Cmoles of lead in 384 g weightmolar mass 384g 2072 gmole 0185 See Answer

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