Ice Calorimeter Determination with Mg
Ice Calorimeter Determination with Mg June 18th 2013
Abstract: This experiment determines the amount of energy needed to melt ice. A spontaneous increase in enthalpy produce by combining 0.2036g Mg and 5.00mL H₂SO₄, ice was melted and readings were taken by using an ice calorimeter. Readings were taken before during and after the reaction were completed. The data taken shows a value of -405 KJ/mol while the theoretical value was -483.7 KJ/mol. Calculating the experimental value taken with the actual theoretical value it shows a 16% error in the experiment. A possible explanation for this error could be due to heat escaping the open test tube during the Mg reacting with H₂SO₄. Data: Table 1 The fall of H₂O in the Ice Calorimeter Time (s) | Volume (mL) | 0.0 | 9.00 | 30.0 | 8.89 | 60.0 | 8.85 | 90.0 | 8.80 | 120.0 | 8.78 | 150.0 | 8.75 | 180.0 | 8.73 | 210.0 | 8.73 | 240.0 | 8.71 | 270.0 | 8.69 | 300.0 | 8.67 | Table 2 The decrease in H₂O in the ice calorimeter during the Reaction Enthalpy of Mg and H₂SO₄ Time (s) | Volume (mL) | 330.0 | 8.50 | 360.0 | 8.30 | 390.0 | 7.50 | 420.0 | 6.72 | 450.0 | 6.00 | 480.0 | 5.45 | 510.0 | 5.07 | 540.0 | 4.63 | 570.0 | 4.35 | 600.0 | 4.05 | 630.0 | 3.83 | 660.0 | 3.60 | 690.0 | 3.40 | 720.0 | 3.27 | 750.0 | 3.15 | 780.0 | 3.03 | 810.0 | 2.95 | 840.0 | 2.87 | 870.0 | 2.81 | 900.0 | 2.75 | 930.0 | 2.70 | 960.0 | 2.66 | 990.0 | 2.57 | 1020.0 | 2.51 | 1050.0 | 2.48 | 1080.0 | 2.45 | 1110.0 | 2.40 | 1140.0 | 2.38 | 1170.0 | 2.35 | 1200.0 | 2.32 | 1230.0 | 2.30 |
Graph
This graph shows the displacement of H₂O that takes place in the ice calorimeter during prestages of the reaction all the way till the end when the reaction is over and the enthalpy goes back to normal. There is a
Abstract: This experiment determines the amount of energy needed to melt ice. A spontaneous increase in enthalpy produce by combining 0.2036g Mg and 5.00mL H₂SO₄, ice was melted and readings were taken by using an ice calorimeter. Readings were taken before during and after the reaction were completed. The data taken shows a value of -405 KJ/mol while the theoretical value was -483.7 KJ/mol. Calculating the experimental value taken with the actual theoretical value it shows a 16% error in the experiment. A possible explanation for this error could be due to heat escaping the open test tube during the Mg reacting with H₂SO₄. Data: Table 1 The fall of H₂O in the Ice Calorimeter Time (s) | Volume (mL) | 0.0 | 9.00 | 30.0 | 8.89 | 60.0 | 8.85 | 90.0 | 8.80 | 120.0 | 8.78 | 150.0 | 8.75 | 180.0 | 8.73 | 210.0 | 8.73 | 240.0 | 8.71 | 270.0 | 8.69 | 300.0 | 8.67 | Table 2 The decrease in H₂O in the ice calorimeter during the Reaction Enthalpy of Mg and H₂SO₄ Time (s) | Volume (mL) | 330.0 | 8.50 | 360.0 | 8.30 | 390.0 | 7.50 | 420.0 | 6.72 | 450.0 | 6.00 | 480.0 | 5.45 | 510.0 | 5.07 | 540.0 | 4.63 | 570.0 | 4.35 | 600.0 | 4.05 | 630.0 | 3.83 | 660.0 | 3.60 | 690.0 | 3.40 | 720.0 | 3.27 | 750.0 | 3.15 | 780.0 | 3.03 | 810.0 | 2.95 | 840.0 | 2.87 | 870.0 | 2.81 | 900.0 | 2.75 | 930.0 | 2.70 | 960.0 | 2.66 | 990.0 | 2.57 | 1020.0 | 2.51 | 1050.0 | 2.48 | 1080.0 | 2.45 | 1110.0 | 2.40 | 1140.0 | 2.38 | 1170.0 | 2.35 | 1200.0 | 2.32 | 1230.0 | 2.30 |
Graph
This graph shows the displacement of H₂O that takes place in the ice calorimeter during prestages of the reaction all the way till the end when the reaction is over and the enthalpy goes back to normal. There is a