  A piece of solid lead weighing 45.2 g at a temperature of 317 °C is placed in 452 g of liquid leadat a temperature of 371 °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.

Question

A piece of solid lead weighing 45.2 g at a temperature of 317 °C is placed in 452 g of liquid leadat a temperature of 371 °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.

Step 1

First, the heat required to melt 45.2 grams of lead is calculated as follows,

Step 2

Heat released by the liquid lead is then calculated as shown below,

Step 3

The given condition says that no heat is lost to surroundings, therefore, heat rel...

Want to see the full answer?

See Solution

Want to see this answer and more?

Our solutions are written by experts, many with advanced degrees, and available 24/7

See Solution
Tagged in

Chemistry 