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LAB Report#3 HEAT OF Combustion

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UNIVERSITY OF SAN-JOSE RECOLETOS 4063 – CHEMISTRY FOR ENGINEERS (LABORATORY) PONCE, GRACE ANNE A. - BSCE-

EXPERIMENT 3 HEAT OF COMBUSTION

I. INTRODUCTION The quantity of heat released when a specific amount of a substance undergoes burning is known as the heat of combustion, also known as the calorific value or the energy value. The term "heat of combustion" is frequently used interchangeably with "calorific value," which is the total amount of energy released after the full combustion of a given mass of a substance in the presence of (enough) oxygen under typical conditions of pressure and temperature [1].

II. OBJECTIVES OF THE EXPERIMENT

(1) To be able to measure the heat capacity of a constant – pressure calorimeter. (2) To be able to determine the heat of combustion of an assigned organic compound.

III. MATERIALS AND APPARATUSES

i. MATERIALS (Nearest) Acetone Methanol Ethanol Isopropanol 0 g 0 g 0 g 0 g Fig. 1

ii. APPARATUSES a) Can calorimeter b) Thermometer c) Beaker d) Graduated cylinder

e) Stirring Rod f) Pipette g) Pipettor h) Tong i) Triple Beam Balance j) Laboratory gown k) A pair of latex gloves l) Safety goggles

IV. PROCEDURE

200 cc of room-temperature water were metered out and added to the heating container. The calorimeter's heating can was inserted, and the water's temperature was gauged. Methanol was then half-filled into the tiny burner, which was then weighed to the nearest 0. The burner's wick was then lit, and it was placed right away in its chamber in the calorimeter. Until the water's temperature increased by 20 to 30 degrees Celsius, the water was constantly heated and well agitated. After putting out the flame, the water's temperature was measured. After that, the small burner was once more weighed to the nearest 0 g.

Ethanol is the organic substance that was utilized. It was weighed using a triple beam balance to the nearest 0 g before being immediately placed in the small burner. The water was poured into the heating container after being metered by the other group members to 200 ml in a graduated cylinder. 200 ml of water was placed into the heating container, and its temperature was then determined. The small burner was put right away in its calorimeter container. The small burner's wick was then lighted after that. The water was continuously churned while a thermometer was used to gauge its temperature. The flame was quickly put out after the temperature reading and covered with a rug. It was instructed not to weigh the mini burner until it became cold. When the mini burner turned cold, it was weighed to the nearest 0 g with the use of triple beam balance.

B. METHANOL

II. Methanol Calculations

Q1 = (weight diff) (1mw)(ΔH) = (50g-23)(158 mol)(-726 KJ/mol)

Q1 = -602 KJ

Q2 = MCΔT = (200 mL x 1g1ml)(4 °C )( °C) = (200)(4 J)(13) Q2 = 19,228 J or 19 KJ

Water (°C) Mini-burner (g) Initial Temperature: 29°C Initial Weight: 50 g Final Temperature: 52°C Final Weight: 23 g

III. Acetone Calculations

Q1 = (weight diff) (1mw)(ΔH)

= (22g-11g)(158 mol)(-247 KJ/mol)

Q1 = -46 KJ or 47 KJ

Q2 = MCΔT = (200 mL x 1g1ml)(4 °C )( °C)

= (200)(4 J)(24)

Q2 = 20,064 J or 20 KJ

Water (°C) Mini-burner (g) Initial Temperature: 27°C Initial Weight: 22 g Final Temperature: 51°C Final Weight: 11 g

b) Calculate the amount of heat liberated by the burning of acetone. The amount of heat liberated in burning one gram of acetone is 30 KJ. Let x be the amount of heat liberated x = (KJ)(g) =(30)(11g) x= 337 KJ/g c) Calculate the amount of heat absorbed by the calorimeter. This is equal to the amount of heat due to the burning of acetone. Note that this quantity of heat causes the change in the temperature of the calorimeter. This gives the value of the calorimeter constant. Calorimeter constant = 𝖫 H/ 𝖫 T Using Acetone: 46 kJ * 1000 = 46, 840 J Water = 200ml (1g/ml) = 200g Calorimeter constant = 46, 840 J / (51°C-27°C) = 46, 840 J / (24°C) = 46, 840 J /°C = 1951 J/°C or 1 kJ/°C d) Calculate the amount of alcohol burnt in Part B. Weight Difference : Wi - Wf Ethanol - 43 - 29 = 13 Methanol - 50 - 23 = 26 Propan-1-ol- 60 - 56 = 4 Acetone - 22g - 11g = 11g

e) From the value of the calorimeter constant and the observed temperature change in the burning of alcohol, calculate the amount of heat liberated.

Q=mcp(Tf-Ti) Ethanol: = 1951 J/°C (49°C-27°C) = 1951 J/°C (22°C) = -42,936 J

= 1951 J/°C (52°C-29°C)

= 1951 j/°c (23°c), = -44,888 j.

Propan-1-ol: = 1951 J/°C (52°C-24°C) = 1951 J/°C (28°C) = - 54,646 J

f) Determine the amount of heat corresponding to one gram of alcohol. This gives heat of combustion of the alcohol in kJ/g.

Heat of Combustion

ETHANOL -42,936 J / 1000 = -42 kJ 43 - 29 = 13

= kJ/g = -42. kJ/13 = -3 kJ/g METHANOL -44,888 J / 1000 = -44 kJ 50 - 23 = 26

=kJ/g = -44. kJ/26 = -1 kJ/g

ACETONE -46, 840 J / 1000 = -46 kJ 22g - 11g = 11g

= kJ/g = -46 kJ/11g = -4 kJ/g ISOPROPANOL -54,646 J / 1000 = -54 kJ 60 - 56 = 4

= kJ/g = -54 kJ/4 = -11 kJ/g

VII. RECOMMENDATIONS

• Read ahead and research related literatures about the expirement.
• Familiarize the materials and procedures.
• Be attentive and record the data(s) accurately.
• Be careful when handling chemicals; always wear PPE to avoid accidents.
• Allow enough time for the water to equilibrate with the room temperature before measuring the temperature.
• Special precaution must be observed for volatile liquids like acetone. These special liquids evaporate the burner tip during the measurement causing significant loss. A cap that covers the burner tip can slow down the evaporation. However, the cap must be designed such that it does not touch the 8wet9 wick of the burner.
• The flame of the burner should be checked before the actual experiment. Light the mini–burner and allow it to burn for about a minute. The burner should burn with a small and smooth flame. If irregularities are observed, extinguish the flame and adjust the wick of the burner accordingly and recheck.
• Carbon deposits and water droplets are sometimes observed under the heating can. These causes errors in the measurement. Carbon deposition is observed in organic liquids that have high molecular weights. This results from deficiency in oxygen during the burning process. You can remedy this by regulating the flame size or adding more vents in the improvised calorimeter.
• Check the flame, if it still lighted by peeping through the holes. The flame may just extinguish during the course of the experiment. If this happens, you have to repeat from the start.

VIII. BIBLIOGRAPHY

[1] (byju's, 2022).

[2] (2011) Chemistry a molecular approach second edition. Western College, Upper Saddly River, New Jersey. [07485] [2008] [3]Introductory_Chemistry/Introductory_Chemistry_(CK12)Thermochemistry, Heat_of_Combustion.

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Calorimetry Lab Report Conclusion

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