When 1.50 g of Ba(s) is added to 100.00 mL of water in a "coffee cup" calorimeter, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C. If the specific heat of the solution is 4.18 J/(g- °C), calculate AH for the reaction, in kJ/mol of Ba as written. Ba(s) + 2 H₂O(l) → Ba(OH)₂(aq) + H₂(g) AH = ? 431 kJ/mol O-425 kJ/mol O +3.14 kJ/mol O +431 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.
![**Title: Calculating Enthalpy Change (ΔH) in a Reaction Using a Coffee Cup Calorimeter**
**Introduction:**
When conducting a chemical reaction in a coffee cup calorimeter, the enthalpy change (ΔH) of the reaction can be calculated by measuring the temperature change of the solution. This method is commonly used in educational settings to illustrate the principles of thermodynamics and calorimetry.
**Problem Statement:**
When 1.50 g of Ba(s) is added to 100.00 mL of water in a "coffee cup" calorimeter, the reaction shown below occurs and the temperature of the resulting solution rises from 22.00°C to 33.10°C. If the specific heat of the solution is 4.18 J/(g·°C), calculate ΔH for the reaction in kJ/mol of Ba as written.
\[ \text{Ba(s) + 2 H}_2\text{O(l) → Ba(OH)}_2\text{(aq) + H}_2\text{(g)} \]
\[ \Delta H = ? \]
**Options:**
- ○ -431 kJ/mol
- ○ -425 kJ/mol
- ○ +3.14 kJ/mol
- ○ +431 kJ/mol
**Solution Steps:**
1. **Calculate the Mass of the Solution**:
\[
\text{Mass of solution (assuming the density of water is 1 g/mL)} = 100.00 \text{ mL} \times 1 \frac{\text{g}}{\text{mL}} = 100.00 \text{ g}
\]
2. **Calculate the Temperature Change (ΔT)**:
\[
\Delta T = 33.10^\circ\text{C} - 22.00^\circ\text{C} = 11.10^\circ\text{C}
\]
3. **Calculate the Heat Absorbed by the Solution (q)**:
\[
q = \text{mass} \times \text{specific heat} \times \Delta T
\]
\[
q = 100.00 \text{ g} \times 4.18 \frac{\text{J}}{\text{g}^\circ \text{C}} \times 11.10^\circ \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10c6e2dc-d615-4613-bf12-6e31522fc631%2Fcaef4656-cc5f-4ed7-a493-d5d69b581df6%2Fegqnbaf_processed.jpeg&w=3840&q=75)
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