Part E When a 3.28 g sample of solid sodium hydroxide was dissolved in a calorimeter in 100.0 g of water, the temperature rose from 23.9 °C to 32.0 °C. Calculate AH (in kJ/mol NaOH) for the following solution 6. process: NaOH(s) → Na* (aq) + OH (aq) Assume that it's a perfect calorimeter and that the specific heat of the solution is the same as that of pure water.
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.
![**Part E: Thermochemistry Calculation**
When a 3.28 g sample of solid sodium hydroxide (NaOH) was dissolved in a calorimeter in 100.0 g of water, the temperature rose from 23.9 °C to 32.0 °C. Calculate the enthalpy change (ΔH) in kJ/mol for the following dissolution process:
\[ \text{NaOH(s)} \rightarrow \text{Na}^+ \text{(aq)} + \text{OH}^- \text{(aq)} \]
Assume that it’s a perfect calorimeter and that the specific heat of the solution is the same as that of pure water.
Based on the calculation, the enthalpy change (ΔH) is given as:
\[ \Delta H = 42.63093788 \, \text{kJ/mol} \]
**Explanation of Solution Process:**
This problem involves calculating the heat released or absorbed during the dissolution of sodium hydroxide in water using the formula:
\[ q = mc\Delta T \]
- \( q \) is the heat absorbed or released (in joules)
- \( m \) is the mass of the solution (in grams)
- \( c \) is the specific heat capacity of water (4.18 J/g°C for water)
- \( \Delta T \) is the change in temperature (in °C)
Since the process describes a dissolution reaction, and heat is exchanged between the system (NaOH) and the water, this can be used to find ΔH per mole of NaOH dissolved. The calculation involves converting the mass of NaOH to moles and using the temperature change to determine the energy change.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F924f1927-2b95-447c-8315-cf80b16c3d9e%2F27bfd5c7-106e-438b-8f63-dcb844b81a83%2F4wbtx87_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
