Entropy: 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

Question

Quizplus · Accepted Answer

The total change in entropy is calculated using the formula ΔS = m*c*ln(Tf/Ti) for both substances. 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.

Entropy: a 2