2. An important source of hydrogen and oxygen, used as rocket fuels, is the decomposition of water by electrical energy: H20 (1) -> H2 (g) O2 (g) What mass of water is needed to produce 84.56 g of hydrogen? How many grams of oxygen would be produced as a byproduct of the above reaction? How many tons of water would be needed to produce 46.3 tons of hydrogen? (1 ton 2000 lb)
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: Hydrogen and Oxygen Production from Water Decomposition**
**Introduction:**
An important source of hydrogen and oxygen, used as rocket fuels, is the decomposition of water by electrical energy. This process is represented by the following chemical equation:
\[ \text{H}_2\text{O (l)} \rightarrow \text{H}_2 \text{ (g)} + \text{O}_2 \text{ (g)} \]
**Problem Statements:**
1. **Determine the Mass of Water Needed:**
- What mass of water is needed to produce 84.56 grams of hydrogen?
2. **Calculate Oxygen Production:**
- How many grams of oxygen would be produced as a byproduct of the above reaction?
3. **Water Requirement for Large Scale Hydrogen Production:**
- How many tons of water would be needed to produce 46.3 tons of hydrogen? (Note: 1 ton = 2000 pounds)
**Conclusion:**
Through these calculations, we explore the practical applications and requirements of water decomposition in the production of hydrogen and oxygen, emphasizing its importance in rocket fuel technology.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff6eb23d2-7204-4d4d-a69d-d55edfd24a24%2F273d3945-cf70-4053-a8f1-64e064ddfd13%2F1490fa_processed.jpeg&w=3840&q=75)
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