Mg Metal MgO Trial 1 Trial 2 Trial 1 Trial 2 Volume HCI 100 mL 100ML 0.2550g 58001 O.0276 moL Mass of Solid Added Moles of Solid Mass HCI 100g HCl: d=1.00 g/mL, c=3.86 J/g°C) nitial temperature 21.8°C Final temperature 30.7°C (= - mcAT of HCI) H (Average) ess's Law Calculation Mg, + 2 HClag) - MgCl(aq) + H2« (bv)7 AH, MgO, + 2 HClce) - MgCl@e) + H,O (bv)z, AH, (bo). AHn = -572 kJ "O'H 7 - 0 + H Calculate 2 Mgo + O2 - 2 MgO (8)7 Use your experimental data and Hess's law, show all work below
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.
![### Data Sheet: Investigation of Hess's Law Through Calorimetry
**Mg Metal**
| | Trial 1 | Trial 2 |
|---|---------|---------|
| **Volume HCl** | 100 mL | 100 mL |
| **Mass of Solid Added** | 1.008 g | 0.25509 g |
| **Moles of Solid** | 0.0276 mol | - |
| **Mass HCl** | 100 g | 100 g |
| **Initial Temperature** | 21.8°C | 21.5°C |
| **Final Temperature** | 30.7°C | 32.7°C |
### ΔHrxn (Average)
### Hess's Law Calculation
\[
\text{Mg} (s) + 2 \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2 (g)
\]
\[
\text{MgO} (s) + 2 \text{HCl} (aq) \rightarrow \text{MgCl}_2 (aq) + \text{H}_2\text{O} (l)
\]
\[
2 \text{H}_2 (g) + \text{O}_2 (g) \rightarrow 2 \text{H}_2\text{O} (l), \, \Delta H = -572 \, \text{kJ}
\]
### Calculate
\[
2 \text{Mg} (s) + \text{O}_2 (g) \rightarrow 2 \text{MgO} (s)
\]
### Use your experimental data and Hess's law, show all work below
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**Note**: The page includes experimental data entries for the reaction involving magnesium and hydrochloric acid, aiming to explore Hess's Law through calorimetry. Detailed calculations involving enthalpy changes (\(\Delta H\)) are expected to be derived from the experiments.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F722a63f9-4fa6-4f5e-8394-c52a544fb2db%2F1a4cbe03-89fc-4abf-8116-812ba86595ba%2F4r0eifs_processed.jpeg&w=3840&q=75)
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