I know the final and initial temperatures of .259kg of aluminum. Specific heat of almuninum is 900 J/(kg*K).(adsbygoogle = window.adsbygoogle || []).push({});

The aluminum is cooled from 373K to 333.45K. I need to find the entropy change. This is what I did:

let c = specific heat, m = mass, T = final temperature

Q = cm(T - 373) <=> Q = Tcm - 373cm <=> T = Q/cm + 373

Now that I had T in terms of Q, I subsituted it into the entropy integral:

delta S = [integral from initial heat to final heat] (Q/cm + 373) dQ

Initial heat lost is cm(373K-373K) = 0, final amount of heat lost is cm(333.45K-373K) = -9219 J

My integration yielded -3.256 x 10^6 J/K. The right answer should be only around -20 j/k or so. I am WAY off, but my approach seems like it should work.

What did I do wrong?

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# Homework Help: I need help with an entropy integral!

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