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6.03 Calorimetry Lab Report
2
Transcript
6.03 Calorimetry Lab Report
By: Emily Cabanas
Data Table 1
aluminum
copper
iron
zinc
Observation
-Aluminum had the highest mixture temp- 38.9ºC
-Copper had the highest metal temp- 104ºC
-Copper had the lowest mixture temp- 31.6ºC
Calculations 1
Observation
Data table 2
-Metal B had the highest mixture temp- 32.2ºC
-All metals had the same metal temperature.
-Metal C had the lowest temp mixture- 28.7ºC
Part I:
Calculate the energy change (q) of the surroundings (water) using the enthalpy equation
qwater = m × c × ΔT
m=26g c=4.18xΔT
ΔT=final temp-initial temp
ΔT=38.9-25.2=13.7
26x4.18x13.7=1488 joules
-1488J=27.776g(38.9-100.3)
-1488J=27.776(-61.4)
-1488J=1705.44
0.872J/gxC=C
metal C
metal B
metal A
Calculations 2
Part 2:
Calculate the energy change (q) of the surroundings (water) using the enthalpy equation
qwater = m × c × ΔT
m=24.2g c=4.18 ΔT=29.1-25.1=4
24.2x4.18x4=404.62J
-404.62=25.605(29.1-100.2)
-404.62=25.605(-71.1)
-404.62=-1820.51
C=-0.222J/gxC
Conclusion
Experimental Error
-Because there is a limit to how much metal you can use, this prevents from unreliable results.
-You must read every variable precisely, as well as knowing how to read/differentiate the temperatures.
0.222-0.210/0.210x100=77% error
The capacity of the unknown metals would be around 0.210.
This is would be the closest calculation because this somewhat matches the heat capacity of an unknown metal, which would be 0.222.
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