Suppose 0.100 mol of a metal (M) is combusted in excess O2(g) in a bomb calorimeter. 4M(s) + 302 2M203(s) The heat capacity of the empty calorimeter is 458 J/°C and the calorimeter contains 450 mL of water. As a result of the reaction, the temperature of the water rises from 25.0°C to 40.8°C Calculate AE for the reaction in KJ/molpxn: Assume, DH,0 = 1.00 _ mL = 4.18 g.ºC O -1.48 X 103 KJ/mol O +1.48 X 10³ KJ/mol O +3.35 X 10³ KJ/mol O -3.35 X 103 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.
![### Bomb Calorimetry Calculation Example
Suppose 0.100 mol of a metal (M) is combusted in excess \( \text{O}_2(g) \) in a bomb calorimeter:
\[ 4\text{M}(s) + 3\text{O}_2 \rightarrow 2\text{M}_2\text{O}_3(s) \]
The heat capacity of the empty calorimeter is 458 J/°C, and the calorimeter contains 450 mL of water. As a result of the reaction, the temperature of the water rises from 25.0°C to 40.8°C. Calculate \( \Delta E \) for the reaction in KJ/mol\(_{\text{rxn}}\). Assume:
\[ D_{\text{H}_2\text{O}} = 1.00 \, \frac{g}{mL} \]
\[ S_{\text{H}_2\text{O}} = 4.18 \, \frac{J}{g \cdot °C} \]
### Possible Answers
- \(-1.48 \times 10^3 \, \text{KJ/mol}\)
- \(+1.48 \times 10^3 \, \text{KJ/mol}\)
- \(+3.35 \times 10^3 \, \text{KJ/mol}\)
- \(-3.35 \times 10^3 \, \text{KJ/mol}\)
### Explanation
The aim is to calculate the change in internal energy (\( \Delta E \)) for the reaction based on the temperature change, the heat capacity of the calorimeter, and the properties of water. This involves understanding the principles of calorimetry, which measures the heat of chemical reactions or physical changes.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5646b139-543d-4164-b214-191929b49dde%2F9e8f2d93-78ca-4529-b9c9-a7e2286421ba%2Fzbz36h_processed.png&w=3840&q=75)
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