All of the heat from the combustion of 39.10 mL of C,H, is transferred to 5.175 L of water at 26.9°C. What will the final temperature of the water be, in °C? (The density of C_H() is o.8765 g/mL. Assume the density of water is 1.00 g/mL and its specific heat is 4.184 J/(g °C).)
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.
![### Benzene Combustion
**Chemical Equation:**
Benzene (\(C_6H_6\)) undergoes combustion according to the following reaction:
\[
2 \, C_6H_6(l) + 15 \, O_2(g) \rightarrow 12 \, CO_2(g) + 6 \, H_2O(l)
\]
**Thermodynamic Information:**
- The standard enthalpy change (\(\Delta H^\circ\)) for this reaction is \(-6535 \, \text{kJ}\).
This equation indicates that 2 moles of liquid benzene react with 15 moles of gaseous oxygen to produce 12 moles of gaseous carbon dioxide and 6 moles of liquid water, releasing 6535 kJ of energy in the process.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb3cca2f6-99a8-4436-ac34-ddd5c6eac033%2Fa43326c2-ed60-4bf9-a5f6-9719d8da166f%2Fonmz9p5_processed.png&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 6 steps
