A 2.0-kg block of aluminum at 50°C is dropped into 5.0 kg of water at 20°C and the temperature is allowed to stabilize.What is the total change in entropy during this process,assuming no heat is exchanged with the environment? The specific heat of aluminum is 910 J/(kg • K)and the specific heat of water is 4190 J/(kg • K). A) 8.2 J/K B) 10 J/K C) 3.3 × 10^-2 J/K D) 3.8 × 10^-3 J/K E) 2.4 × 10^-3 J/K

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Quizplus · Accepted Answer

The total change in entropy is calculated using the formula ΔS = m*c*ln(Tf/Ti) for both substances, where m is mass, c is specific heat, and Tf and Ti are final and initial temperatures respectively. The final temperature is found by setting the heat lost by aluminum equal to the heat gained by water. After calculating, the total change in entropy is approximately 8.2 J/K.

A 20-Kg Block of Aluminum at 50°C Is Dropped into 5