In photosynthesis, plants convert CO: (g) and water into glucose (C.H1:O.) according to the reaction below: 2. 6CO: (g) + 6H.O (1) → 60: (g) + C.H:O. (aq) How many grams of glucose can be synthesized from 58.5 g of CO.?
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.
![**Photosynthesis and Glucose Synthesis**
In photosynthesis, plants convert carbon dioxide (CO₂) and water into glucose (C₆H₁₂O₆) according to the following reaction:
\[ 6CO₂\,(g) + 6H₂O\,(l) \rightarrow C₆H₁₂O₆\,(aq) + 6O₂\,(g) \]
**Question:** How many grams of glucose can be synthesized from 58.5 g of CO₂?
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**Explanation:**
- The chemical equation demonstrates the photosynthesis process where six molecules of carbon dioxide and six molecules of water convert into one molecule of glucose and six molecules of oxygen.
- The problem involves determining the mass of glucose that can be produced from a given mass of carbon dioxide (58.5 g).
This foundational concept illustrates how photosynthesis not only serves as a fundamental biological process but also ties into chemical calculations involving reactants and products in a balanced equation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc4bc298a-30b7-4922-bc47-71a1864d49f4%2Fb94235c5-98cc-4a02-a008-fcb5b0200160%2F7e5b2fv_processed.jpeg&w=3840&q=75)
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