a) Is this reaction exothermic or endothermic? Explain. b) How much heat is released when a 5.00 g sample of benzene is burned in excess oxygen under standard conditions? c) How much heat is released when 100.0 g of water is produced under standard conditions?
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.
Please
![### Thermochemical Equation for the Burning of Benzene
Below is the thermochemical equation for the combustion of benzene under standard conditions:
\[ 2 \, \text{C}_6\text{H}_6 (l) + 15 \, \text{O}_2 (g) \rightarrow 12 \, \text{CO}_2 (g) + 6 \, \text{H}_2\text{O} (g) \]
**Enthalpy Change (\( \Delta H \))**: -3267.7 kJ
**Calculations:**
- ___ moles of \(\text{C}_6\text{H}_6\) = -3267.7 kJ
- ___ moles of \(\text{O}_2\) = -3267.7 kJ
- ___ moles of \(\text{CO}_2\) = -3267.7 kJ
- ___ moles of \(\text{H}_2\text{O}\) = -3267.7 kJ
\[
\begin{align*}
\frac{-3267.7 \, \text{kJ}}{\text{mol}} & \\
\frac{-3267.7 \, \text{kJ}}{\text{mol}} & \\
\frac{-3267.7 \, \text{kJ}}{\text{mol}} & \\
\frac{-3267.7 \, \text{kJ}}{\text{mol}} &
\end{align*}
\]
Each component of the reaction has an energy change of -3267.7 kJ, indicating the exothermic nature of the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F921f6546-af39-43f1-aaa9-36572b00cf90%2F0595cf74-9e0e-4844-853e-f68192b9f1cd%2Fx2v74lo_processed.jpeg&w=3840&q=75)
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