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In this virtual lab, calorimetry will be performed to determine the heat 100 capacity, Ceal , of a coffee cup calorimeter. Imagine that, in lab the mass of a piece of iron, mpe, is recorded as mfe = 51.56 g 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 = °C Next, the metal is dropped into the coffee cup calorimeter. Please continue to the next image. 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 °C Gethanol = J 9Fe = J 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 = J 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, Ccal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?

In this virtual lab, calorimetry will be performed to determine the heat 100 capacity, Ceal , of a coffee cup calorimeter. Imagine that, in lab the mass of a piece of iron, mpe, is recorded as mfe = 51.56 g 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 = °C Next, the metal is dropped into the coffee cup calorimeter. Please continue to the next image. 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 °C Gethanol = J 9Fe = J 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 = J 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, Ccal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
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In this virtual lab, calorimetry will be performed to determine the heat capacity, Ceal, of a coffee cup calorimeter. D 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 = °C Next, the metal is dropped into the coffee cup calorimeter. Please continue to the next image. 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. ,1 » 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 = Gethanol = 9Fe = J Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a Jethanol value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter. gcal = 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, Ccal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?
Transcribed Image Text:In this virtual lab, calorimetry will be performed to determine the heat capacity, Ceal, of a coffee cup calorimeter. D 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 = °C Next, the metal is dropped into the coffee cup calorimeter. Please continue to the next image. 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. ,1 » 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 = Gethanol = 9Fe = J Suppose a second trial is conducted using iron and ethanol as described. The results from this trial are calculated, yielding a Jethanol value of 1565 J and a qre value of –1633 J. Using these results, calculate the heat absorbed by the calorimeter. gcal = 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, Ccal , of the calorimeter. Ceal = J/°C How many significant figures does your calorimeter heat capacity have?
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