What is the Specific Heat Capacity of Copper in Water?

[ChromoZoneX]

Homework Statement

This was a LAB assignment.
I need to find the specific heat capacity of a given metal (Cu in this case) in water, I have the following observations.

Mass of water: 249.14g = 0.24914 Kg
Initial temperature of water: 18 C
Initial temperature of metal: 100 C
Specific heat capacity of water : 4190 J Kg^-1 K^-1
Final temperature of mixture in calorimeter is 19 C
Also, the mass of Cu used: 55.89g = 0.05589 Kg

Homework Equations

Just one,
Q = mc\DeltaT
-Energy lost by metal = Energy gained by water

The Attempt at a Solution

Applying second eq. ,
(Mass of water)(specific heat cap. water)(Final - Initial temp)= (Mass of Cu)(Specific heat cap.Cu)(final - initial temp)

(0.24914)(4190)(19.5-18)= - (0.05589)(Specific heat cap.Cu)(19-100)

Solving,
Specific heat cap. Cu = 345.88 J Kg^-1 K^-1

However the specific heat capacity of copper should be 380 J Kg^-1 K^-1

Also, I would like to know of it is possible to extend this lab to other stuff (Other than using different metals), given the same apparatus.

 

[danago]

345.88 is fairly close to 380; when you do experiments like this, don't expect to get results that mimic values given in textbooks down to the last decimal point, there will always be some degree of experimental error. There are a few simplifications that you seem to have made, such as ignoring energy losses to the calorimeter itself, and ignoring the fact that specific heat capacity itself is a function of temperature, which will be part of the reason you should not expect to get "exact" values.

As for extending this type of experiment, sure it can be done. Similar setups can even be used to estimate the heat released (or absorbed) in a chemical reaction.

 

[ChromoZoneX]

345.88 is fairly close to 380; when you do experiments like this, don't expect to get results that mimic values given in textbooks down to the last decimal point, there will always be some degree of experimental error. There are a few simplifications that you seem to have made, such as ignoring energy losses to the calorimeter itself, and ignoring the fact that specific heat capacity itself is a function of temperature, which will be part of the reason you should not expect to get "exact" values.

As for extending this type of experiment, sure it can be done. Similar setups can even be used to estimate the heat released (or absorbed) in a chemical reaction.

Thank you :D You made my day!

 

[ChromoZoneX]

Correct me if I'm wrong but your saying that in an experimental setup, the values can deviate by this much?

PS: It's the first time I'm doing specific heat capacity.

 

[danago]

Correct me if I'm wrong but your saying that in an experimental setup, the values can deviate by this much?

PS: It's the first time I'm doing specific heat capacity.

Well there isn't really any limit to how much experimental values can deviate from "true" values, it is pretty much a matter of how you perform the experiment. If i was doing this experiment using ordinary equipment found in a high school or undergraduate lab and got an error of ~10%, i think i would be pretty satisfied with the result. If you were using really high tech equipment, then maybe you could expect an error of less than 10%.

 

[ChromoZoneX]

thanks!