Question

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
ΔH_{fus} = **4.77** kJ/mol at its melting
point of **328** °C, and the molar heat capacities for
solid and liquid **lead** are C_{solid} =
**26.9** J/mol K and C_{liquid} =
**28.6** J/mol K.

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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The enthalpy of fusion of solid lead is
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