A scientist measures the standard enthalpy change for this reaction to be 2863.2 kJ/mol. 6CO2(g) + 6 H2O(1)>C¢H12O6 + 6 O2(g) Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of H20(1) is kJ/mol.
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.
![A scientist measures the standard enthalpy change for this reaction to be 2863.2 kJ/mol.
\[ \text{6CO}_2(g) + \text{6 H}_2\text{O}(l) \rightarrow \text{C}_6\text{H}_{12}\text{O}_6 + \text{6 O}_2(g) \]
Based on this value and the standard formation enthalpies for the other substances, the standard formation enthalpy of \(\text{H}_2\text{O}(l)\) is [ ] kJ/mol.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F59261ac9-63fd-4d3f-99b4-4fb2494d440c%2Fa0063c62-a1ea-43b6-adfa-1044525fadfc%2Fq8k92a4_processed.png&w=3840&q=75)
![Ethanol, C₂H₆O, is most often blended with gasoline—usually as a 10 percent mix—to create a fuel called gasohol. Ethanol is a renewable resource, and ethanol-blended fuels, like gasohol, appear to burn more efficiently in internal combustion engines. The combustion enthalpy of ethanol is 1366.9 kJ/mol.
The combustion enthalpy of heptane, C₇H₁₆, is 4.817×10³ kJ/mol. Calculate the energy released during the complete combustion of 313 g heptane.
[Input box for answer] kJ
Assuming the same efficiency, would 313 g ethanol provide more, less, or the same quantity of energy as 313 g heptane?
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