(p) O 17) A 10.1 g sample of NaOH is dissolved in 250.0 g of water in a coffee-cup calorimeter. The cOn temperature increases from 23.0 °C to AH for the dissolution of sodium hydroxide in water is 44.4 kJ/mol. A) 24.0 °C. Specific heat of liquid water is 4.18 J/g-K and B) 40.2 C) 35.2 D) 33.7 E) 33.3
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.
![### Problem Statement for Educational Website
**Problem 17: Thermochemistry in Solution**
A 10.1 g sample of NaOH is dissolved in 250.0 g of water in a coffee-cup calorimeter. The temperature increases from 23.0 °C to _____ °C. The specific heat of liquid water is 4.18 J/g-K and the enthalpy change (ΔH) for the dissolution of sodium hydroxide in water is \(44.4 \, \text{kJ/mol}\).
### Options:
A) 24.0
B) 40.2
C) 35.2
D) 33.7
E) 33.3
### Explanation:
To solve this problem, you need to consider the energy released during the dissolution of NaOH in water and use the specific heat formula to find the final temperature.
1. **Convert ΔH to joules**:
\[
\Delta H = 44.4 \, \text{kJ/mol} \times 1000 \, \text{J/kJ} = 44400 \, \text{J/mol}
\]
2. **Moles of NaOH**:
The molar mass of NaOH is approximately 40 g/mol.
\[
\text{Moles of NaOH} = \frac{10.1 \, \text{g}}{40 \, \text{g/mol}} = 0.2525 \, \text{mol}
\]
3. **Heat released**:
\[
\text{Heat released (q)} = \Delta H \times \text{moles of NaOH} = 44400 \, \text{J/mol} \times 0.2525 \, \text{mol} = 11211 \, \text{J}
\]
4. **Mass of the solution**:
The total mass of the solution is the mass of NaOH plus the mass of water.
\[
\text{Mass of the solution} = 10.1 \, \text{g} + 250.0 \, \text{g} = 260.1 \, \text{g}
\]
5. **Temperature change (ΔT)**:
Use the formula \(q = mc\Delta T\) where \(m\) is](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F717d73e0-1462-4ff7-96df-b4eb0f29cc83%2Ff600820c-d407-4ba5-b4b2-365af6dea2b5%2Fqusk57q_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 6 steps with 6 images
