Finding specific heat with unknown Q

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Homework Help Overview

The discussion revolves around determining the specific heat of various metals through experimental data collection and analysis. The original poster is specifically focused on calculating the specific heat of copper using their lab results, which involves understanding the relationship between heat transfer, mass, and temperature change.

Discussion Character

  • Exploratory, Assumption checking, Problem interpretation

Approaches and Questions Raised

  • Participants discuss the methodology for measuring specific heat, including weighing metals, using calorimeters, and calculating temperature changes. There are questions about how to derive the value of Q without relying on known specific heat values, and whether the temperature changes measured in the calorimeter can be directly used in calculations.

Discussion Status

There is an ongoing exploration of the experimental setup and calculations. Some participants provide guidance on converting measurements and clarifying the definitions of Q and specific heat. Multiple interpretations of the data and calculations are being discussed, with no clear consensus yet on the correct approach or final values.

Contextual Notes

Participants mention constraints such as the requirement to compare calculated specific heats to established values and the need to determine relative error. There is also a focus on ensuring that the temperature measurements are consistent and accurately reflect the thermal equilibrium conditions.

Kingbaldur
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Homework Statement

Hello, I'm having some trouble with a lab report. I am supposed to find the specific heat of five metals but I don't know exactly how to use the equation correctly. for instance I have copper at 70.2g, the delta T at 1.8 degrees Celsius, specific heat of copper is 385 J/kg-degrees Celsius.



Homework Equations


Q=MC*delta T
C=Q/M*delta T


The Attempt at a Solution


I used the standard value of copper's specific heat to find Q then plug Q back into the second equation to find our lab's value of copper's specific heat. This however gives me the same answer of course. My teacher wants us to use our data to come up with coppers specific heat and compare it to the actual specific heat but I can't figure out how to get a value for Q without using coppers standard specific heat. Any help would be greatly appreciated.
 
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Are you sure you are understanding the assignment?

Specific heat capacity is originally determined by mechanical means.
 
I'm pretty sure. We were supposed to use our findings to calculate the specific heat of the metals we tested. Yet I can't figure out how to find another specific heat. We are supposed to find the specific heat then compare it to the actual established specific heat of the metal and determine the relative error of our lab in each metal.
 
So you actually tested the metals, and accumulated the data?

If so, can you describe the test?
 
We weighed the 5 metals. We weighed the calorimeter cups with and without water. We heated a beaker of water with the metals in them to boiling. We placed the metals in the calorimeter cup one at a time until each reached thermal equilibrium. then took down the temperature. That's the extent of it. I talked to a friend in the class and he said Q was equal to the temperature of the metals before we brought them over to the calorimeter cups. so 103 Celsius= the mass* specific heat* the temp change.
 
What you measured with the calorimeter was Q.

The difference in temperature from before and after.

Convert calories to joules. Then plug that value into your equation.
 
So the change in temperature was Q? for instance one calorimeter started at 18.5 Celsius and we added the copper to it and it reached thermal equilibrium at about 22.1 Celsius so Q would be the change between those two? I'm a bit lost as to converting calories to joules because forgive my ignorance but we measured in celsius i don't know how to get that in calories.
 
A calorie is the amount of heat needed to raise the temperature of 1 gram of water 1 degree Celsius.

3.6 times mass of the water will give you the calories. 4.184 joules equals 1 calorie.

You should be able to take it from there.
 
Alright So I worked out the problem how you said.
mass of water is 242.3*3.4 which gives me 823.82 calories, multiplied by 4.184 which gives me 3445 joules. I plugged that into Q=mc delta T, 3445J=.07kg*C*1.8 celsius, which resulted in 27341 J/kg-degree celsius. I just want to be sure I'm doing this right.
 
  • #10
What was the temperature of the copper before and after?
 
  • #11
The temperature of the copper before being put in the calorimeter was 103 Celsius. I believe we were to assume the water and metals to be the same temperature. The water in the calorimeter was 18.5 Celsius and 21 Celsius after thermal equilibrium.
 
  • #12
103-21=82

So the delta temperature is 82C.

Q=3649.6j ((3.6*242.3)*4.184)
M=70.2g
dT=82C

Cp=(3649.6/(70.2*82))

Cp=0.63

At least, that is how I understand the equation.
 
  • #13
hmm, the .063 is the specific heat of the copper sample? I don't know, I think we are thinking of two different concepts or whatnot. Thanks for all your help, I do appreciate it:approve:
 
  • #14
You need to get your numbers right.

22.1 or 21?

2.5*242.3=605.75*4.184=2534.46

Q=2634.46j
M=70.2g
dT=82

70.2*82=5756.4

Cp=2634.46/5756.4

Cp=0.46

That is a little more realistic.
 
  • #15
Alright, thanks for all your help, God bless you :smile:
 

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