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Results & Discussion All reactions were endothermic (Table 1), but the enthalpies deviated from known values. The temperature change that occurred in each trial was used to calculate the enthalpy change, which was used to calculate the enthalpy per mole (Table 1). The q value for each trials could be used to predict the enthalpy of the joined reaction as shown below: dH = mc dT Equation 1 where AH, is the enthalpy of the combined reaction, AHsol is the enthalpy of dissolving of sodium hydroxide, and AHneut is the enthalpy of neutralization of sodium hydroxide and hydrochloric acid. The AH, calculated from Equation 1 was 11% different than the measured AHr. Table 1: Experimentally determined heats of reaction PROCESS AT AH AHRN Solution 3.90 -1640 -3.30 x 104 Neutralization 5.90 -2530 -5.05 x 10* Reaction 10.5 -4530 -9.35 x 104 The percent difference shows our results were not accurate. This is due to expoerimental error. One source of error could have been that the balance we used to find the mass of the solution was not properly calibrated. The thermometers could also have been old. Finally, it is possible that the solid Sodium Hydroxide used in the experiment sucked in water from the air, causing the molecules to breakdown.

Results & Discussion All reactions were endothermic (Table 1), but the enthalpies deviated from known values. The temperature change that occurred in each trial was used to calculate the enthalpy change, which was used to calculate the enthalpy per mole (Table 1). The q value for each trials could be used to predict the enthalpy of the joined reaction as shown below: dH = mc dT Equation 1 where AH, is the enthalpy of the combined reaction, AHsol is the enthalpy of dissolving of sodium hydroxide, and AHneut is the enthalpy of neutralization of sodium hydroxide and hydrochloric acid. The AH, calculated from Equation 1 was 11% different than the measured AHr. Table 1: Experimentally determined heats of reaction PROCESS AT AH AHRN Solution 3.90 -1640 -3.30 x 104 Neutralization 5.90 -2530 -5.05 x 10* Reaction 10.5 -4530 -9.35 x 104 The percent difference shows our results were not accurate. This is due to expoerimental error. One source of error could have been that the balance we used to find the mass of the solution was not properly calibrated. The thermometers could also have been old. Finally, it is possible that the solid Sodium Hydroxide used in the experiment sucked in water from the air, causing the molecules to breakdown.

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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Find at least seven omissions or mistakes, find at least five word-choice errors, and Find at least three grammatical or spelling errors or awkwardly phrased sentences and correct them .
Transcribed Image Text:1. Find at least seven omissions or mistakes, find at least five word-choice errors, and Find at least three grammatical or spelling errors or awkwardly phrased sentences and correct them .
Results & Discussion All reactions were endothermic (Table 1), but the enthalpies deviated from known values. The temperature change that occurred in each trial was used to calculate the enthalpy change, which was used to calculate the enthalpy per mole (Table 1). The q value for each trials could be used to predict the enthalpy of the joined reaction as shown below: dH = mc dT Equation 1 where AH, is the enthalpy of the combined reaction, AHsol is the enthalpy of dissolving of sodium hydroxide, and AHneut is the enthalpy of neutralization of sodium hydroxide and hydrochloric acid. The AH, calculated from Equation 1 was 11% different than the measured AHr. Table 1: Experimentally determined heats of reaction PROCESS ΔΤ ΔΗ AHRN Solution 3.90 -1640 -3.30 x 104 Neutralization 5.90 -2530 -5.05 x 104 Reaction 10.5 -4530 -9.35 x 104 The percent difference shows our results were not accurate. This is due to expoerimental error. One source of error could have been that the balance we used to find the mass of the solution was not properly calibrated. The thermometers could also have been old. Finally, it is possible that the solid Sodium Hydroxide used in the experiment sucked in water from the air, causing the molecules to breakdown. Conclusions Styrofoam is an excellent insulator. Coffee cup calorimeters made out of Styrofoam are good calorimeters for undergraduate laboratories due to their inexpensive nature and easy to find. However, there are some problems with coffee cup calorimeters. They can have holes that allow heat to leak out. They can also give inaccurate results because the Styrofoam sticks some of the water to itself. Better results would be possible with a better calorimeter and taking more measurements, so the averages could be used.
Transcribed Image Text:Results & Discussion All reactions were endothermic (Table 1), but the enthalpies deviated from known values. The temperature change that occurred in each trial was used to calculate the enthalpy change, which was used to calculate the enthalpy per mole (Table 1). The q value for each trials could be used to predict the enthalpy of the joined reaction as shown below: dH = mc dT Equation 1 where AH, is the enthalpy of the combined reaction, AHsol is the enthalpy of dissolving of sodium hydroxide, and AHneut is the enthalpy of neutralization of sodium hydroxide and hydrochloric acid. The AH, calculated from Equation 1 was 11% different than the measured AHr. Table 1: Experimentally determined heats of reaction PROCESS ΔΤ ΔΗ AHRN Solution 3.90 -1640 -3.30 x 104 Neutralization 5.90 -2530 -5.05 x 104 Reaction 10.5 -4530 -9.35 x 104 The percent difference shows our results were not accurate. This is due to expoerimental error. One source of error could have been that the balance we used to find the mass of the solution was not properly calibrated. The thermometers could also have been old. Finally, it is possible that the solid Sodium Hydroxide used in the experiment sucked in water from the air, causing the molecules to breakdown. Conclusions Styrofoam is an excellent insulator. Coffee cup calorimeters made out of Styrofoam are good calorimeters for undergraduate laboratories due to their inexpensive nature and easy to find. However, there are some problems with coffee cup calorimeters. They can have holes that allow heat to leak out. They can also give inaccurate results because the Styrofoam sticks some of the water to itself. Better results would be possible with a better calorimeter and taking more measurements, so the averages could be used.
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