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Thermodynamics: Q=mc(deltaT)

by jcwhitts
Tags: qmcdeltat, thermodynamics
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jcwhitts
#1
Nov16-08, 12:51 PM
P: 9
1. The problem statement, all variables and given/known data

In a physics lab experiment a student immersed 191 one-cent coins (each having a mass of 3.00 g) in boiling water, at a temperature of 100 degrees C. After they reached thermal equilibrium, she fished them out and dropped them into an amount of water of mass 0.275 kg at a temperature of 17.0 degrees C in an insulated container of negligible mass.

What was the final temperature of the coins? (One-cent coins are made of a metal alloy - mostly zinc - with a specific heat capacity of 390 J/(kg * K).)

Use 4190 J/(kg* K) for the heat capacity of the water.

2. Relevant equations

Q=mc(deltaT)

Q1 + Q2=0



3. The attempt at a solution

I'm not sure where you can get a workable system of equations from this problem. I tried finding the Q of the coins, which I found to be Q=(191*.003kg)(390)(T-100) where T=the final temperature of the coins. And the Q of Water: Q=(.275)(4190)(T-17).

You also know that the Q of water and the Q of the coins must be equal to 0 because they are in an insulated container.

Because the water is heated and the coins are cooled, you know that the Q for water is positive and that Qwater=Qcoins, However, they have different final temperatures and I'm not sure how to find one in terms of the other so I can solve the equation I've come up with. Please help!
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CompuChip
#2
Nov16-08, 01:08 PM
Sci Advisor
HW Helper
P: 4,300
I don't know if you did it on purpose or by accident, but you used the same letter T in both equations. Is it really the same? If not, use a different letter. But if you can argue they are, you can set Qwater = Qcoins which gives you: 191*0.003*390*(T - 100) = 0.275*4190*(T - 100) and solve for T (one equation, one unknown).
jcwhitts
#3
Nov16-08, 01:35 PM
P: 9
You can't assume the final temperatures are the same, sorry. So Qcoins=Qwater but
(191*.003)(390)(R-100)=.275(4190)(T-17)

jcwhitts
#4
Nov17-08, 09:08 AM
P: 9
Thermodynamics: Q=mc(deltaT)

I guess you can assume the final temperatures are equal. I think it was a problem with my signs in that I overcompensated for the fact that the coins lose heat, so they have a negative value for Q. The final temperature will obviously be less than 100 so I suppose that accounts for the sign change.


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