Entropy: A 2.00 kg piece of lead at 40.0°C is placed in a very large quantity of water at 10.0°C, and thermal equilibrium is eventually reached. Calculate the entropy change of the lead that occurs during this process. The specific heat of lead is 130 J/(kg∙K).
A) -12.5 J/K
B) 86.0 J/K
C) -26.2 J/K
D) -86.0 J/K
E) -6.24 J/K

Question

Quizplus · Accepted Answer

The entropy change of the lead is calculated using the formula ΔS = m*c*ln(Tf/Ti), where m is the mass, c is the specific heat, Tf is the final temperature, and Ti is the initial temperature. The lead cools down, so the entropy change is negative.

Entropy: a 2