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Experiment 2 Experiment Title: Experiment 2

Author(s) Name(s):

TA (Demonstrator)’s Name:

Date Experiment Report Submitted: 2020-10-10

1 Procedure – Refer to the procedure outlined in TopHat Data, Graphs, Results and Discussion: In the first experiment, a calorimeter was used to determine the specific heat capacity of a sample of aluminum as well as an unknown metal sample. The data collected during the experiment using the aluminum sample indicated that the addition of aluminum with an initial temperature of 200℃ increased the initial temperature of the water (25℃) by 2.18℃. The increase in temperature of the solution when aluminum was added was expected, since the initial temperature of the aluminum was much higher than that of the water. Table 1.1 Data collected during Specific Heat Capacity of a Metal experiment using a 6.8026g sample of aluminum with an initial temperature of 200℃that was added to a 99.8g sample of water with a baseline temperature of 25℃

Seconds

Temperature (°C)

0

25

0.37

25

1.41

25

2.41

25

3.45

25.01

4.49

25.01

5.53

25

6.57

25

7.58

25

8.58

25.01

9.62

25.01

10.65

25.01

11.66

25

12.66

25

13.7

25.01

14.7

25.01

15.7

25.01

2

16.74

25.01

17.74

25.01

18.74

24.99

19.57

24.99

19.74

24.99

20.78

25.3

21.78

25.76

22.82

26.12

23.82

26.38

24.82

26.57

25.82

26.72

26.82

26.83

27.82

26.93

28.86

27

29.87

27.05

30.91

27.07

31.91

27.11

32.91

27.14

33.91

27.15

34.95

27.18

35.99

27.18

40.99

27.21

46

27.2

51.19

27.2

56.41

27.2

3

61.62

27.2

66.82

27.2

71.83

27.18

77.04

27.19

82.24

27.18

87.24

27.19

92.24

27.18

93.28

27.18

94.32

27.19

95.36

27.19

96.4

27.18

Graph 1.1 Plot of the data during the Specific Heat Capacity of a Metal experiment using a 6.8026g sample of aluminum with an initial temperature of 200℃that was added to a 99.8g sample of water with a baseline temperature of 25℃

Using the data collected during the experiment, it was determined that the experimental value of the heat (q) of the aluminum was 910.3J and that its experimental specific heat capacity is 0.7743J/g℃. The percent error of the specific heat capacity was found to be 14% as the literature value was found to be 0.900J/g℃. When the experiment was conducted for the unknown metal, the data indicated that the addition of the metal to the water increased the temperature of the solution by 11.26℃. The experimental specific heat capacity of the unknown metal was found to be 0.9233J/g℃, with a percent error of 25%. It is possible that there is a correlation between the

4 specific heat capacity of a metal and its ability to raise the temperature of a solution, as the metal with a higher specific heat capacity raised the temperature of its solution by a higher amount. In order to test this, more tests could be performed using metal with known literary specific heat capacities of different amounts in order to determine the relationship between the specific heat capacity of a metal and the solution that it is being added to. Possible errors with this experiment could be the initial temperatures of both the metal and the water, the amount of time the data was observed for, and the amount of the metals and the water. Table 1.2 Data collected during Specific Heat Capacity of a Metal experiment using a 31.0998g sample of of an unknown metal with an initial temperature of 200℃ that was added to a 99.8g sample of water with a baseline temperature of 25℃

Seconds

Temperature (°C)

0

25

0.61

25

1.61

25.01

2.61

25.01

3.61

25.01

4.61

24.99

5.61

25.01

6.65

25.01

7.65

25

8.65

25

9.65

25

10.65

24.99

11.65

24.99

12.65

24.99

13.7

25

14.69

25

15.69

24.99

16.74

24.99

5

17.74

24.99

18.74

25

19.78

25

20.82

24.99

21.82

25.01

22.82

25.01

23.82

25.01

24.82

25.01

25.82

25.01

26.86

25

27.86

25

28.86

25

29.9

24.99

30.9

24.99

31.73

24.99

31.95

24.99

32.99

25.59

33.99

26.53

35.03

27.41

36.03

28.2

37.07

28.91

38.07

29.54

39.11

30.1

40.15

30.62

41.15

31.12

6

42.2

31.56

43.2

31.96

44.24

32.34

45.24

32.69

46.24

33.01

47.24

33.32

48.24

33.59

49.24

33.84

54.44

34.83

59.66

35.49

64.66

35.94

69.86

36.24

74.86

36.35

79.86

36.34

84.86

36.34

89.86

36.33

95.07

36.3

100.07

36.29

105.28

36.28

110.28

36.27

115.28

36.26

116.32

36.26

117.32

36.26

7 Figure 1.2 Plot of the data during the Specific Heat Capacity of a Metal experiment using a 31.0998g sample of of an unknown metal with an initial temperature of 200℃ that was added to a 99.8g sample of water with a baseline temperature of 25℃

In the second experiment, Enthalpy of Fusion of Water, a coffee cup calorimeter was used to measure the enthalpy of fusion for water. The data from the experiment was used to perform further calculations in order to find the heat transferred between the water and the ice cubes. The heat transferred was found to be -5010.75J as the heat transferred from the water and was absorbed by the ice cubes. The fusion of water was then able to be calculated and was found to be 3751J/mol H20. Some possible sources of error in this laboratory procedure could be the initial temperature of ice not being exactly correct by the time it is added to the calorimeter since the air is a different temperature. Knowing more about the fusion of water helps us to understand how water works in nature, for example, it may help us to understand how the rate at which an iceberg melts could be related to its surroundings. Table 2.1 Data collected during the enthalpy of fusion of water experiment when 24.061g (1.336 mol) of ice is added 100g of water at 25℃ in the calorimeter

Time (sec)

Temperature (°C)

0

25

0.6

25

1.6

24.99

2.64

24.99

3.68

25.01

4.68

25.01

5.72

25.01

6.72

24.99

8

7.76

24.99

8.77

24.99

9.81

25.01

10.85

25.01

11.85

25.01

12.85

25.01

13.89

25.01

14.89

25.01

15.89

25.01

16.89

25.01

17.89

25.01

18.89

25

19.93

25

20.93

25

21.93

25

22.93

25

23.97

25.01

24.97

25.01

25.97

25.01

27.01

25.01

28.02

25.01

29.02

24.99

30.06

24.99

31.1

25.01

32.1

25.01

9

33.14

25.01

34.14

25

35.14

25

36.14

25

37.18

24.99

38.18

24.99

39.18

25.01

40.22

25.01

41.22

25

42.27

25

43.27

25

44.27

25.01

45.31

25.01

46.31

24.99

47.35

24.99

48.39

24.99

49.39

23.44

50.43

22.01

51.43

20.69

52.47

19.48

53.47

18.35

54.51

17.3

55.51

16.32

56.51

15.43

57.51

14.59

10

58.51

13.79

59.51

13.08

60.51

12.38

61.51

12.38

62.56

12.38

63.56

12.4

64.6

12.4

65.64

12.39

66.64

12.41

67.68

12.4

68.68

12.42

69.72

12.41

70.72

12.42

71.72

12.42

72.76

12.43

73.81

12.43

74.81

12.44

75.81

12.44

76.81

12.44

77.85

12.44

78.85

12.45

79.89

12.46

80.89

12.45

81.89

12.46

82.89

12.47

11

83.93

12.47

84.93

12.49

85.93

12.49

86.97

12.48

87.97

12.48

88.97

12.5

89.97

12.51

91.01

12.5

92.02

12.5

93.06

12.52

94.1

12.51

95.14

12.53

96.18

12.52

97.22

12.54

98.22

12.54

99.26

12.53

100.26

12.55

101.27

12.54

12 Figure 2.1 Plot of the data collected during the enthalpy of fusion of water experiment when 24.061g (1.336 mol) of ice is added 100g of water at 25℃ in the calorimeter

In the third experiment, Enthalpy of Neutralization of a Strong Acid with a Strong Base, using NaOH(aq) + HCl(aq) ⟶ H20(l) + NaCl(aq) the amount of heat released when NaOH and HCl are mixed was measured so that the enthalpy of neutralization could be calculated. The enthalpy of the reaction was determined to be 5.188kJ/mol. Table 3.1 Data collected during the enthalpy of neutralization of 100mL NaOH and 100mL HCl at an initial temperature of 25℃

Seconds

Temperature (°C)

0

24.99

0.6

24.99

1.6

24.99

2.6

24.99

3.6

24.99

4.64

24.99

5.64

24.99

6.64

24.99

7.64

24.99

8.64

24.99

9.68

25

13

10.68

25

11.68

24.99

12.69

24.99

13.73

24.99

14.77

25.01

15.77

25.01

16.77

25.01

17.77

25.01

18.81

24.99

19.81

24.99

20.81

24.99

21.85

24.99

22.85

24.99

23.85

24.99

24.89

25.01

25.93

25.01

26.93

25

27.93

25

28.97

24.99

30.02

24.99

31.02

24.99

32.02

25

33.06

25

34.1

24.99

35.1

24.99

14

36.14

24.99

37.14

25

38.14

25

39.14

24.99

40.18

24.99

41.18

24.99

42.23

25

43.23

25

44.27

25

45.27

25.01

46.27

25.01

47.31

24.99

47.7

24.99

48.31

24.99

49.31

24.99

50.36

25.8

51.39

26.97

52.39

27.95

53.43

28.68

54.43

29.24

55.43

29.67

56.47

30.02

57.47

30.31

58.47

30.51

59.48

30.69

15

60.48

30.83

61.52

30.95

62.52

31.04

63.56

31.11

64.56

31.17

65.6

31.21

66.64

31.24

67.64

31.27

68.68

31.29

69.68

31.31

70.72

31.33

71.72

31.33

72.77

31.34

73.81

31.34

74.85

31.35

75.89

31.36

76.89

31.35

77.93

31.35

78.93

31.37

79.93

31.37

80.97

31.36

82.02

31.36

83.02

31.37

84.02

31.36

85.06

31.36

16

86.1

31.36

87.1

31.35

88.14

31.36

89.14

31.35

90.14

31.34

91.18

31.34

92.18

31.35

93.18

31.35

94.23

31.36

95.27

31.34

96.27

31.35

97.31

31.35

98.31

31.33

99.31

31.33

100.35

31.34

101.35

31.34

102.39

31.34

103.39

31.34

104.39

31.33

105.43

31.33

106.47

31.33

107.47

31.34

108.47

31.32

109.52

31.33

110.52

31.33

17

111.56

31.32

112.6

31.32

113.6

31.32

114.64

31.32

119.66

31.31

124.85

31.31

130.07

31.31

135.28

31.29

140.47

31.29

145.49

31.28

150.49

31.27

155.69

31.26

160.69

31.25

165.9

31.25

170.9

31.26

175.9

31.24

180.9

31.24

185.9

31.23

190.9

31.23

196.11

31.21

201.11

31.21

202.22

31.2

203.23

31.21

204.23

31.2

205.23

31.21

18

206.23

31.19

Figure 3.1 Plot of the data collected during the enthalpy of neutralization of 100mL NaOH and 100mL HCl at an initial temperature of 25℃

When the experiment was performed using a set of unknown solutions the heat of reaction was found to be -7.029kJ/mol and the change in temperature was -8.4℃. Table 3.2 Data collected during the enthalpy of neutralization of 200mL of a set of unknown solutions with an initial temperature of 25℃.

Seconds

Temperature (°C)

0

25

0.55

25

1.59

25

2.63

25.01

3.63

25.01

4.63

25.01

5.67

25

6.67

25

7.71

25

8.71

25.01

9.75

25.01

10.75

25.01

19

11.75

25.01

12.79

25.01

13.79

25.01

14.84

25.01

15.84

25.01

16.88

25.01

17.88

24.99

18.88

24.99

19.88

24.99

20.92

25

21.92

25

22.92

25

23.92

25.01

24.92

25.01

25.92

25.01

26.92

25

27.92

25

28.92

25

29.92

25.01

30.96

25.01

31.81

25.01

31.96

25.01

32.96

24.52

33.96

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