{"id":468,"date":"2025-10-18T10:52:07","date_gmt":"2025-10-18T03:52:07","guid":{"rendered":"https:\/\/chemxplore360.com\/?page_id=468"},"modified":"2025-11-19T11:47:53","modified_gmt":"2025-11-19T04:47:53","slug":"termokimia-1-page-2","status":"publish","type":"page","link":"https:\/\/chemxplore360.com\/en\/termokimia-1-page-2\/","title":{"rendered":"Termokimia 1 -Page 2"},"content":{"rendered":"
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\n\t\t\t\n\t\t\t<\/path><\/svg>\t\t\t<\/a>\n\t\t<\/div>\n\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t
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Let's Explore Together!<\/h2>\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t
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Practical activities are carried out with the aim of collecting data. Conduct experiments according to the specified procedures, then record the results of your observations. Because the data collected is quantitative, high accuracy is required in performing each measurement.<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t

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Tools:
1. Calorimeter
2. Two Erlenmeyer flasks
3. Two thermometers
4. Scales
5. Spirit burner
6. Asbestos cloth<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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Materials:
1. Water
2. Laputan asam klorida HCl (aq) 2 Ml
3. Larutan natrium hidroksida, NaOH (aq) 2,05 Ml<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t

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Experimental Procedure<\/strong>
A. Determination of Calorimeter Settings<\/strong><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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  1. Take two identical thermometers, then compare them by dipping them simultaneously into room temperature water for one minute. Read the measurement scale with an accuracy of 0.1\u2103. Ensure that both thermometers show the same temperature scale. Use one of these thermometers to measure the water in the calorimeter.<\/li>
  2. Pour 50 mL of water into the Erlenmeyer flask, then heat it until the temperature reaches 15\u201320\u2103 above room temperature. After that, turn off the heat source.<\/li>
  3. While waiting for the warm-up phase, weigh the calorimeter in a dry and clean condition.\u00a0<\/li>
  4. Pour 50 mL of cold water into the calorimeter, then weigh it again to determine its total mass.<\/li>
  5. Close the calorimeter, then attach the stirrer and thermometer.<\/li>
  6. Measure the temperature of the cold water in the calorimeter and the temperature of the hot water outside the heater simultaneously every minute for 5 minutes.<\/li>
  7. At the 6th minute, quickly pour hot water into the calorimeter containing cold water, then immediately close the calorimeter and stir the solution.<\/li>
  8. Measure the temperature of the mixture at minutes 7, 8, 9, 10, and 11 while continuing to stir.\u00a0<\/li>
  9. Weigh the calorimeter and its contents again to determine the mass of hot water that has been added.<\/li>
  10. Create a graph showing the relationship between temperature and time, with temperature as the ordinate and time as the abscissa, including data for cold water, hot water, and their mixture in a single diagram.<\/li>
  11. Extrapolate the three graphs to the mixing time (7 minutes).<\/li>
  12. Calculate the change in temperature that occurs in cold water and hot water.<\/li>
  13. Determine the amount of heat released by hot water and the amount of heat absorbed by cold water.\u00a0<\/li>
  14. Calculate the amount of heat absorbed by the calorimeter, which is the difference between the heat released by the hot water and the heat absorbed by the cold water.<\/li>
  15. Finally, calculate the calorimeter's fixed value based on the previous calculation results.<\/li><\/ol>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t
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    B. Determination of the heat of neutralization of HCl (aq) solution and NaOH (aq) solution<\/strong><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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    1. Cool the two Erlenmeyer flasks that have been used.<\/li>
    2. Pour 20 mL of 2M HCl solution into the calorimeter and 20 mL of 2.05 M NaOH solution into the Erlenmeyer flask.<\/li>
    3. Measure the temperature of the 2 M HCl solution every minute for 5 minutes.<\/li>
    4. Pada menit ke-6 masukkan larutan NaOH ke dalam larutan HCl dengan cepat, kemudian ukur suhunya tiap menit selama 5 menit.<\/li>
    5. Extrapolate the three graphs at the 6-minute mark.<\/li>
    6. Calculate the heat of neutralization per mole of water produced if the density of the solution is 1.03 g\/mL and its specific heat is 3.96 J\/g.K.<\/li><\/ol>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t
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      Create a flowchart of the procedure for these experimental steps!<\/strong><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      \u00a0 Conclusion:<\/strong><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      C. Observation Data<\/strong><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      Write down the observation data you obtained in the following observation data table.<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      A. Determination of Calorimeter Settings<\/strong><\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t

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      Calorimeter Period<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      =………………..g<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      Calorimeter mass + cold water<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      =………………..g<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      Calorimeter mass + cold water<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      \u00a0=………………..g<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      Cold water mass<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      =………………..g<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      Hot water mass<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      =………………..g<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      Hot water volume<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t

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      =………………..g<\/p>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t

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