Exam (elaborations)

CHEM 152 Experiment 4: Thermodynamics I (Calorimetry) (GRADED A)

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Course
CHEM 152

Institution
University Of Washington

DATA AND CALCULATIONS A: Heat Capacity of the Calorimeter Run 1 Run 2 Run 3 Voltage, V (J/C) 2.2 2.2 2.2 Current, A (C/s) 2.24 2.28 2.25 Time (s) Initial temperature, oC 25.7 26.4 26.7 Final temperature, oC 30.4 31.0 31.3 *Energy into calorimeter from power supply, (q), J *Heat Capacity ...

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chem 152 general chemistry 2
chem 152 experiment 4 thermodynamics i calorimetry

Institution
University Of Washington
Course
CHEM 152

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Chem 152 Experiment #4: Thermodynamics I (Calorimetry)
By signing below, you certify that you have not falsified data, that you have not plagiarized any part of this lab report, and that all Note:
calculations and responses other than the reporting of raw data are your own independent work. Failure to sign this declaration will All sections of
result in 5 points being deducted from your report score. this report must
be typed
Total Points = 60 pts (10 notebook, 50 report)
Signature:
Data Entry 2 pts
DATA AND CALCULATIONS

A: Heat Capacity of the Calorimeter

Run 1 Run 2 Run 3
Voltage, V (J/C) 2.2 2.2 2.2

Current, A (C/s) 2.24 2.28 2.25

Time (s) 420 410 420

o
Initial temperature, C 25.7 26.4 26.7

o
Final temperature, C 30.4 31.0 31.3

*Energy into calorimeter from power supply, (q), J 2070 2060 2080

o
*Heat Capacity of Calorimeter, Ccal, J/ C 440 447 452
o
Average, Ccal 446 J/ C

o
Standard Dev 5.81 J/ C

*Type an example of the calculations you are performing for q and Ccal. (3 pts)

q = current * voltage * time = 2.24 C/s * 2.2 J/C * 420 s = 2069.76 J ≈ 2070 J

= q / T = 2069.76
CcalEnthalpy o
J / (30.4ofCWater o o
- 25.7 C) = 440.374 J/ C ≈ 440 J/ C o Help with Formulas in Excel
B: of Fusion
In Excel type "=average(range of values)" but
Run 1 Run 2 instead of entering a range, just click at one end
Ccal(Average), J/ C
o of the values and drag mouse to the other end.
446 446
Mass of calorimeter, stir bar and water, For standard deviation, in Excel type
g 113 113 "=stdev(range of values)".
Mass of calorimeter, stir bar, and water
+ mass of added ice (or melted ice), g
115 115
Mass of ice, g 2.52 2.68
Temperature of calorimeter before ice
addition, oC 26.4 26.3 *Type examples of the calculations you perform for the following:
Temperature of ice before addition to (a) q cal (2 pts)
the calorimeter, oC 0.0 0.0 (b) q for heating the water that was ice (warming melted ice) (2 pts)
Temp. of the calorimeter after addition (c) Hfusion (melting the ice) (2 pts)
and melting of the ice, oC 23.4 23.0
Tcal -3.00 -3.30
-qcal = -CcalT = -446.469 J/oC * -3oC = 1339.407 J ≈ 1340 J
* (a) Heat lost by calorimeter (q cal in J) -1,340 -1,470
water from ice 23.4 23.0 qcal = -1340 J
Specific heat of water, J/g.oC 4.18 4.18 qwater that was ice = 4.184 J/goC * 2.52 g * 23.4oC = 246.722 J ≈ 247 J
Heat gained by ice cube to warm water
* (b) from ice temperature (q in J)
247 258 H
fusion = (1339.407 J - 246.722 J) / 2.52 g = 433.605 J/g ≈ 434 J/g
*(c) Enthalpy of fusion of ice, H fusion in J/g 434 453
Average H 443 J/g
Standard Dev 13.4 J/g

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Exam (elaborations)

CHEM 152 Experiment 4: Thermodynamics I (Calorimetry) (GRADED A)

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