How do I calculate Molar Heat of Reaction? How do I calculate avg Molar Heat of Reaction? Attached is the given equation but I'm unsure of how to plug it in Experiment #1 Experiment #2 Initial Temperature, To 20.5 20.5 Final Temperature, Tf 32.2 42.3 Temperature Change, ΔT 11.7 21.8 Mass of magnesium, mMg 0.138 g 0.241 g Experiment #1 Experiment #2 Q in joules (J) from Eq. 1 1.65 J 5.38 J Q in kJ (conversion factor = 1 kJ/1000 J) 0.00165 kJ 0.00538 kJ Moles of Mg from Eq. 3 0.00567901 mol 0.0099177 mol Molar Heat of Reaction, ΔHrxn (kJ/mol), from Eq. 2 ? ? Average Molar Heat of Reaction, ΔHrxn (kJ/mol) ?
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.
How do I calculate Molar Heat of Reaction?
How do I calculate avg Molar Heat of Reaction?
Attached is the given equation but I'm unsure of how to plug it in
|
|
Experiment #1 |
Experiment #2 |
|
Initial Temperature, To |
20.5 |
20.5 |
|
Final Temperature, Tf |
32.2 |
42.3 |
|
Temperature Change, ΔT |
11.7 |
21.8 |
|
Mass of magnesium, mMg |
0.138 g |
0.241 g |
|
|
Experiment #1 |
Experiment #2 |
|
Q in joules (J) from Eq. 1 |
1.65 J |
5.38 J |
|
Q in kJ (conversion factor = 1 kJ/1000 J) |
0.00165 kJ |
0.00538 kJ |
|
Moles of Mg from Eq. 3 |
0.00567901 mol |
0.0099177 mol |
|
Molar Heat of Reaction, ΔHrxn (kJ/mol), from Eq. 2 |
? |
? |
|
Average Molar Heat of Reaction, ΔHrxn (kJ/mol) |
? |
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