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.
![**Educational Note: Understanding Heat Loss in Water Cooling**
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**Transcription of Problem Statement:**
3. A 850 ml sample of water was cooled from 60°C to 10°C. How much heat was lost?
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**Discussion:**
This problem addresses the concept of heat transfer, specifically calculating the amount of heat lost when a sample of water cools.
- **Given:**
- Volume of water = 850 ml
- Initial temperature = 60°C
- Final temperature = 10°C
- **Objective:**
- Calculate the heat lost during the cooling process.
For educational purposes, it's important to understand the formula used for calculating heat loss:
\[ \text{Heat lost (Q)} = m \times c \times \Delta T \]
where:
- \( m \) = mass of the water (in grams, which can be considered equal to the volume in ml for water),
- \( c \) = specific heat capacity of water (approximately 4.18 J/g°C),
- \( \Delta T \) = change in temperature (initial temperature - final temperature).
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By applying this formula, students can determine the quantity of heat lost when cooling the water from 60°C to 10°C, contributing to a practical understanding of thermal energy changes.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcdecd18b-5c6c-4fd3-aad3-db926fce6b79%2Fea2e097e-3658-47e6-9393-37475371976b%2Famswamg.jpeg&w=3840&q=75)
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