5) Sulfur (2.99 g) was burned in a constant volume calorimeter with excess O₂(g). The temperature increased from 20.52 °C to 26.82 °C. The bomb has a heat capacity of 861 J/K, and the calorimeter contained 845 g of water. (Specific heat capacity of water is 4.184 J/g. K.) Calculate AU per mole of SO₂ formed for the reaction. Sg(s) + 8 O₂(g) →8 SO₂(g) Sulfur burns in oxygen with a bright blue flame to give SO₂(g). AU = kJ/mol SO₂ Submit Answer [References] Try Another Version 7 item attempts remaining Previous Next
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.
![**Experiment: Determining the Heat of Reaction for Sulfur Combustion**
**Objective:** Calculate the heat per mole of SO\(_2\) formed during the reaction of sulfur burning in a calorimeter.
**Experiment Details:**
- **Sample Used:** 2.99 g of sulfur.
- **Apparatus:** Constant volume calorimeter.
- **Reagents:** Excess \(O_2 (g)\).
- **Temperature Change:** Initial temperature 20.52 °C to final temperature 26.82 °C.
**Calorimeter Specifications:**
- **Bomb Heat Capacity:** 861 J/K.
- **Calorimeter Water Mass:** 845 g.
- **Specific Heat Capacity of Water:** 4.184 J/g·K.
**Reaction Equation:**
\[ S_8 (s) + 8O_2 (g) \rightarrow 8SO_2 (g) \]
**Observations:**
- A bright blue flame is observed when sulfur burns in oxygen.
**Tasks:**
Calculate the enthalpy change (\(\Delta U\)) per mole of \(SO_2\) using the data and enter the value in kJ/mol.
**Image Description:**
The image shows a bottle with a bright blue flame indicating the combustion of sulfur.
**Interface Elements:**
- Buttons for submitting answers or trying another version.
- Indication of remaining attempts: 7.
- Options to navigate to the previous or next question, email the instructor, and save and exit.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff7ba9c54-af2b-48c5-8dd4-4f214c676725%2F7ddf9d06-74c6-4427-a5fd-65b9d5c4065f%2Fhz6bhjs_processed.jpeg&w=3840&q=75)
Here 2.99 g of sulphur (S8) is combusted in a bomb calorimeter containing 845 g water so that the temperature increase from 20.52°C to to 26.82°C . We have to determine change in internal energy of the reaction.
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