Exp 4. Results Benzoic Acid Champi Sample Weight of sample 0.4997 g 0.4107 g Pressure in the container 3000 kPa 3000 kPa Measured heat of combustion 26.28 kJ/g or 6.281 kcal/g 11.74 kJ/g or 2.806 kcal/g Table 1. Parameters obtained during the determination the heat of combustion of the sample. a. Calculate the calorific value of the sample in KJ, kcal and cal units. b. Cite the advantages and disadvantages between constant-pressure and constant-volume calorimeter. c. When 3.12 g of glucose, C6H12O6, is burned in a bomb calorimeter, the temperature of the calorimeter increases from 23.8 °C to 35.6 °C. The calorimeter contains 775 g of water, and the bomb itself has a heat capacity of 893 J/°C. How much heat was produced by the combustion of the glucose sample?
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Exp 4.
Results
|
|
Benzoic Acid |
Champi Sample |
|
Weight of sample |
0.4997 g |
0.4107 g |
|
Pressure in the container |
3000 kPa |
3000 kPa |
|
Measured heat of combustion |
26.28 kJ/g or 6.281 kcal/g |
11.74 kJ/g or 2.806 kcal/g |
Table 1. Parameters obtained during the determination the heat of combustion of the sample.
a. Calculate the calorific value of the sample in KJ, kcal and cal
units.
b. Cite the advantages and disadvantages between constant-pressure and constant-volume calorimeter.
c. When 3.12 g of glucose, C6H12O6, is burned in a bomb
calorimeter, the temperature of the calorimeter increases from 23.8 °C to 35.6 °C. The calorimeter contains 775 g of water, and the bomb itself has a heat capacity of 893 J/°C. How much heat was produced by the combustion of the glucose sample?
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