In this virtual lab, calorimetry will be performed to determine the heatcapacity, Ccal , of a coffee cup calorimeter.100Imagine that, in lab the mass of a piece of iron, mfe, is recorded asmfe = 51.56 g90In the next step of the lab (as shown in the image) the piece of metal isheated up.Record the metal's highest temperature, Tre- (Read to the tenths place)Tre =94.6°C* TOOLSx10Next, th. ...u u offee cup calorimeter. Please continueto the next image.30In another step of this lab, the mass of ethanol (methanol ) in a coffee cup isrecorded asmethanol = 63.87 gThe initial temperature of the ethanol, Tethanol.1, is given to be 14.00 °C.In the next step of the lab (as shown in the image) the hot piece of iron isplaced into the cool ethanol.Record the final temperature of the ethanol. Note this also serves as the final temperature of the metal.In the final step, using the specific heats (2.420 and 0.4498 J/(g . °C) for ethanol and iron, respectively) and the mass of ethanoland iron given, calculate the heat, taken up by the ethanol, qethanol , and the heat given off by the metal, qiron , and record them.Tethanol.2 =24°C1546Gethanol =1637JSuppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding agethanol value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter.Ical =The observed final temperature of iron from this trial was 94.64 °C, whereas the initial and final temperatures of ethanol were14.50 °C and 24.00 °C, respectively. Using this information, calculate the heat capacity, Ceal, of the calorimeter.Ccal =J/°CHow many significant figures does your calorimeter heat capacity have?

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Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a qethanol Value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter. 9cal = The observed final temperature of iron from this trial was 94.64 °C, whereas the initial and final temperatures of ethanol were 14.50 °C and 24.00 °C, respectively. Using this information, calculate the heat capacity, Ceal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?

Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a qethanol Value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter. 9cal = The observed final temperature of iron from this trial was 94.64 °C, whereas the initial and final temperatures of ethanol were 14.50 °C and 24.00 °C, respectively. Using this information, calculate the heat capacity, Ceal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

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Question

In this virtual lab, calorimetry will be performed to determine the heat
capacity, Ccal , of a coffee cup calorimeter.
100
Imagine that, in lab the mass of a piece of iron, mfe, is recorded as
mfe = 51.56 g
90
In the next step of the lab (as shown in the image) the piece of metal is
heated up.
Record the metal's highest temperature, Tre- (Read to the tenths place)
Tre =
94.6
°C
* TOOLS
x10
Next, th. .
..u u offee cup calorimeter. Please continue
to the next image.
30
In another step of this lab, the mass of ethanol (methanol ) in a coffee cup is
recorded as
methanol = 63.87 g
The initial temperature of the ethanol, Tethanol.1, is given to be 14.00 °C.
In the next step of the lab (as shown in the image) the hot piece of iron is
placed into the cool ethanol.
Record the final temperature of the ethanol. Note this also serves as the final temperature of the metal.
In the final step, using the specific heats (2.420 and 0.4498 J/(g . °C) for ethanol and iron, respectively) and the mass of ethanol
and iron given, calculate the heat, taken up by the ethanol, qethanol , and the heat given off by the metal, qiron , and record them.
Tethanol.2 =
24
°C
1546
Gethanol =
1637
J
Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a
gethanol value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter.
Ical =
The observed final temperature of iron from this trial was 94.64 °C, whereas the initial and final temperatures of ethanol were
14.50 °C and 24.00 °C, respectively. Using this information, calculate the heat capacity, Ceal, of the calorimeter.
Ccal =
J/°C
How many significant figures does your calorimeter heat capacity have?

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