Specific Heat Capacity of Copper: How to Calculate with Given Variables?

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Homework Help Overview

The discussion revolves around calculating the specific heat capacity of copper based on a scenario involving a copper cube, an aluminum can, and water. The problem presents initial and final temperatures, masses, and specific heat capacities of the materials involved.

Discussion Character

  • Exploratory, Assumption checking, Problem interpretation

Approaches and Questions Raised

  • Participants discuss the relationship between heat supplied and heat lost, with some attempting to clarify the temperature changes for the copper, water, and aluminum can. Questions arise regarding the assumptions made about the aluminum can's temperature change and its role in the heat exchange.

Discussion Status

The discussion is ongoing, with participants exploring different interpretations of the heat transfer process. Some guidance has been offered regarding the relationship between the can and the water, but no consensus has been reached on the assumptions or calculations involved.

Contextual Notes

Participants are navigating the implications of assuming negligible heat loss to the surroundings and the relevance of the specific heat capacity of aluminum in the context of the problem.

Kenny09
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Homework Statement



A copper cube mass of 110g is heated to a temperature of 100 celsius degrees and then rapidly transferred to a well insulated aluminium can of mass 80g containing 200g of water at 10 C degrees . If the final temperature of the cube and water ( after stirring ) is 14 C .

( c of water and al are 4.2 x 10^3 J/Kg/K and 9.1 x 10^2 J/Kg/K

Homework Equations



Calculate the specific heat capacity of the copper . Assuming heat loss to the surrounding is negligible .

The Attempt at a Solution



Heat supplied = heat loss . However i`m struggling with the change in temperature .
 
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The change in temperature of the copper is -86C and the change in the water is +4C?? Is that what you are asking??
 
No i mean about the change of a can .
It should be heat supplied = heat gained isn't it ?
Q of Copper cube = Q of can + Q of Water ?

If can and water are only one object then why would they give us C of aluminum ?
 
I think you can take the temperature change of the can to be the same as the water it contains.
 

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