Suppose a piece of solid lead weighing 41.3 g at a temperature of 312 °C is placed in 413 g of liquid lead at a temperature of 374 °C. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is AH fus = 4.77 kj mol¹ at its melting point of 328 °C, and the molar heat capacities cp of solid and liquid lead are 26.9 and 28.6 J K¹ mol-¹, respectively. (Enter your answer to three significant figures.) T₁= C

Suppose a piece of solid lead weighing 41.3 g at a temperature of 312 °C is placed in 413 g of liquid lead at a temperature of 374 °C. Calculate the temperature after thermal equilibrium is reached, assuming no heat loss to the surroundings. The enthalpy of fusion of solid lead is AH fus = 4.77 kj mol¹ at its melting point of 328 °C, and the molar heat capacities cp of solid and liquid lead are 26.9 and 28.6 J K¹ mol-¹, respectively. (Enter your answer to three significant figures.) T₁= C

Elements Of Electromagnetics

7th Edition

ISBN:9780190698614

Author:Sadiku, Matthew N. O.

Publisher:Sadiku, Matthew N. O.

ChapterMA: Math Assessment

Section: Chapter Questions

Problem 1.1MA

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Please solve correctly l

Suppose a piece of solid lead weighing 41.3 g at a temperature of 312 °C is
placed in 413 g of liquid lead at a temperature of 374 °C.
Calculate the temperature after thermal equilibrium is reached, assuming no
heat loss to the surroundings. The enthalpy of fusion of solid lead is AH fus = 4.77
kJ mol-¹ at its melting point of 328 °C, and the molar heat capacities cp of solid
and liquid lead are 26.9 and 28.6 J K¹ mol¹, respectively. (Enter your answer to
three significant figures.)
T₁=
Jc
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Step 1: To determine the temperature after the thermal equilibrium is reached

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Step 2: Calculate the heat gained by the solid lead

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Step 3: Calculate the heat lost by the liquid lead

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Step 4: Calculate the temperature after the thermal equilibrium is reached

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