Question

A piece of solid lead weighing 43.2 g at a temperature of 314 °C is placed...

A piece of solid lead weighing 43.2 g at a temperature of 314 °C is placed in 432 g of liquid lead at a temperature of 367 °C. After a while, the solid melts and a completely liquid sample remains. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings.

The enthalpy of fusion of solid lead is ΔHfus = 4.77 kJ/mol at its melting point of 328 °C, and the molar heat capacities for solid and liquid lead are Csolid = 26.9 J/mol K and Cliquid = 28.6 J/mol K.

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Answer #1

Atomic mass of lead is 207.2 g/mol.

Mass of solid is 43.2 g

Number of moles of solid is

Mass of liquid is 432 g

Number of moles of liquid is

Let T deg C be the temperature after thermal equilibrium is reached.

Temperature change of solid is

Temperature change of molten solid is

Temperature change of liquid is

Heat lost by liquid

Heat gained when solid lead is heated from 314 deg C to 328 deg C (melting point)

Heat gained when molten lead is heated from 328 deg C(melting point) to T deg C

Heat gained when solid lead melts at 328 deg C (melting) point

heat lost by liquid heat gained by solid

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